H
H
1
H
Hydrogen 1.0079
H
H
H
CHEMISTRY Investigate the Matter That Makes Up Your World
INQUIRE AND INVESTIGATE
Carla Mooney
Illustrated by Samuel Carbaugh
Contents Timeline... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . vii Introduction
Chemistry Matters!.. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 1 Chapter 1
Atoms, Elements, and the Periodic Table. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 11
Chapter 2
States of Matter: Gases, Liquids, and Solids. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 23
Chapter 3
Changing States of Matter. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 39
Chapter 4
Compounds, Mixtures, and Solutions.. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 47
Chapter 5
Chemical Reactions. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 65
Chapter 6
Acids and Bases.. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 81
Chapter 7
The Nucleus and Radioactivity.. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 91
Chapter 8
Other Branches of Chemistry. . . . .. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 101 Glossary Metric Conversions Resources Periodic Table Index
Chapter 1
Atoms, Elements, and the Periodic Table
How are atoms, elements, and the periodic table related to each other?
Elements are made of atoms, which are the building blocks of matter. The periodic table is the tool scientists use to organize the different elements according to their properties.
Everything around you is made of matter. But what is matter made of? Matter consists of tiny building blocks called atoms. Atoms can be densely packed together to form a solid object, such as this book. Or atoms can be more spread out and appear as a liquid or a gas. Understanding atoms and how they work is at the heart of chemistry.
PARTS OF AN ATOM Atoms contain three basic parts—protons, neutrons, and electrons. Protons and neutrons exist inside the nucleus of the atom, which is the center of the atom. Electrons stay outside the nucleus. Protons are small particles with positive electrical charges, represented by the plus symbol (+). The number of protons in an atom determines what element it is. For example, an atom with two protons is always an element called helium, while an atom with six protons is an element called carbon.
12
CHEMISTRY | CHAPTER ONE
Neutrons, unlike protons, have no electrical charge. A neutron’s job is to help stabilize the atom. To understand why, think about two magnets and their poles, or ends. If the poles have opposite charges, which means one is positive while the other is negative, they attract each other and pull together. But if the poles have the same charge, both positive or both negative, they repel and push away from each other. In the same way, protons with the same positive charge repel each other. Neutrons act like peacemakers, keeping the protons collected together and stabilizing the atom’s nucleus.
Together, an atom’s protons and neutrons make up most of its mass. Electrons are small, negatively charged particles that exist outside of the atom’s nucleus. We use the minus symbol (-) to represent an electron. The opposite charges of the electron and proton attract each other, just as opposite magnetic poles attract each other. This force holds the atom together. The positive charge of one proton and the negative charge of one electron cancel each other out. Therefore, an atom with the same number of protons and electrons will have no charge and will be neutral. While the number of protons in an atom does not change, some special atoms can have more or fewer electrons. These are called ions. An atom that gains electrons becomes negatively charged and is called an anion. An atom that loses electrons becomes positively charged and is called a cation. The “t” in the word cation makes a plus sign to remind us it’s positive.
Electrons are very small compared to the rest of the atom. In fact, the mass of an electron is more than 1,000 times smaller than the mass of a proton. Sticky Atoms Have you ever rubbed a balloon against your head and had it stay there even after you let it go? Static electricity happens because electrons and protons attract and repel each other. When you rub that balloon on your head, electrons transfer from your head to the balloon. The balloon now has more electrons than protons, giving it a negative charge. Your head has lost some electrons, giving it a positive charge. The negatively charged balloon is attracted to the positive charge on your head. Try it!
ATOMS, ELEMENTS, AND THE PERIODIC TABLE
13
ATOMIC ORBITALS
CHEMISTRY CONNECTION Electrons fill the lowest energy levels first, and also fill the orbitals in a specific order. The electron filling pattern is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f. Knowing this pattern can help in some areas of chemistry.
So where exactly are an atom’s electrons? The answer is actually pretty complicated. Electrons are always moving, spinning in clouds around the atom’s nucleus. Because electrons move so quickly, chemists cannot see where they are at any specific moment. Scientists used to believe that electrons orbited the nucleus of an atom like planets around the sun. With more research, they discovered that this idea was too simple. Chemists now believe that there are specific areas where electrons are likely to be found. An atom’s electrons are located in energy levels, numbered 1, 2, 3, and so on. Energy levels are different distances from the atom’s nucleus. Energy level 1 is the closest to the nucleus, while the highest number energy level is the farthest away. An electron spinning in the first energy level will always be closer to the nucleus than an electron spinning in the second energy level. The more electrons an atom has, the more energy levels it has. Inside each energy level, there are spaces where electrons are likely to be located. These spaces are called orbitals. Chemists have named electron orbitals with letters, such as s, p, d, f, and g.
14
CHEMISTRY | CHAPTER ONE
Orbitals are different shapes. For example, the s orbital is shaped like a sphere, while the p orbital is shaped like a dumbbell. Electrons usually fill the lowest energy levels first. If electrons were filling a theater to see a performance, they would all take seats in the front row until it was full, then move on to the second row, and so on. There is a limit to the number of electrons that can inhabit each energy level. The first energy level holds up to two electrons, and the second energy level can hold up to eight electrons. The formula 2 × n2, where n = the energy level, can be used to figure out how many electrons each energy level can hold. Using this formula, we know that the third energy level can hold up to 18 electrons (2 × 32 = 18).
WHAT IS AN ELEMENT? Thousands of years ago, ancient Greek philosophers believed that all matter was made from combinations of just four elements—earth, water, air, and fire. Although we know today that they were wrong, the idea that elements are the basis of all matter is actually true. An element is something that cannot be broken down into a simpler substance. It is something that is made up of only one type of atom. To date, scientists have discovered 118 different elements. These 118 elements combine to make millions of different substances.
Electron Configuration To describe the electrons in an atom, scientists use a notation called an electron configuration: n (type of orbital) number of electrons A hydrogen atom has only one electron, which can be found in the first energy level (1), in the s orbital. Its electron configuration can be written as 1s1 and looks like this:
H
The atom beryllium has four electrons, two in the first energy level and two in the second. Therefore, beryllium’s electron configuration is 1s2 2s2. It looks like this:
Be
Some elements, such as gold, copper, and carbon, have been known for thousands of years. Others, such as livermorium, have been discovered recently. In the future, even more elements might be discovered.
ATOMS, ELEMENTS, AND THE PERIODIC TABLE
15
THE PERIODIC TABLE History of the Periodic Table In 1869, a Russian chemist named Dmitri Mendeleev was the first to publish a periodic table similar to the one we use today. It’s said that he used to play a kind of solitaire on long train rides using cards with information about the elements written out on them. This helped him figure out how to group the elements together in a chart. You can see Mendeleev’s original table here. You can see an interactive version of the periodic table we use today here. Watch videos about every element in the periodic table! endeleev periodic table • PBS M periodic table • periodic videos
16
CHEMISTRY | CHAPTER ONE
The atoms that make up all known elements are organized on a chart called the periodic table of elements. It is organized in a grid, with rows and columns. You can use the large periodic table on page 117 as a reference for the rest of the book. Each element on the periodic table is located in a specific square based on its atomic structure and characteristics. Each square displays certain information about that element, including its element name, symbol, atomic number, and atomic mass. Every element is represented by one or two letters called its atomic symbol. For example, the element lithium’s atomic symbol is Li, while the element carbon’s atomic symbol is C. Iron is Fe. Every element also has an atomic number. For example, lithium’s atomic number is 3. Carbon’s is 6. The periodic table lists elements in the order of their atomic number, from left to right and top to bottom. An element’s atomic number tells you how many protons are in that atom’s nucleus. In a lithium atom, which has an atomic number of 3, there are three protons. In a carbon atom, there are six protons. Because neutral atoms have the same number of protons and electrons, an element’s atomic number can also tell you how many electrons it has. Therefore, a lithium atom also has three electrons and a carbon atom has six electrons. Each square on the periodic table also shows the element’s average atomic mass. Elements are so tiny that it does not make sense to measure them in kilograms or even grams. Scientists use a unit of measurement called an amu (atomic mass unit) to measure the mass of an atom.
1
2
H
hydrogen 1.0079
3
Li
lithium 6.941
11
4
Be
beryllium 9.0122
12
Na Mg sodium 22.990
19
K
potassium 39.098
37
magnesium 24.305
20
Ca Sc calcium 40.078
38
Rb Sr rubidium 85.468
55
strontium 87.62
56
Cs Ba
caesium 132.91
87
scandium 44.956
39
Fr Ra radium [226]
22
Y
57–71
72
yttrium 88.906
Metalloids
Transitional Metals
Non-metals
Other Metals
Noble Gases
Ti
23
V
vanadium 50.942
41
24
25
26
27
28
B
6
Al
14
boron 10.811
13
30
31
Si
15
carbon 12.011
aluminium 26.982
29
C
7
silicon 28.086
32
N
8
P
16
nitrogen 14.007
S
17
oxygen 15.999
phosphorus 30.974
33
O
9
sulfur 32.065
34
niobium 92.906
73
Hf Ta
104
tantalum 180.95
105
F
10
Cl
18
fluorine 18.998
chlorine 35.453
35
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
chromium 51.996
42
manganese 54.938
43
iron 55.845
44
cobalt 58.933
45
nickel 58.693
46
copper 63.546
47
zinc 65.38
48
gallium 69.723
49
germanium 72.64
50
arsenic 74.922
51
selenium 78.96
52
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
zirconium 91.224
hafnium 178.49
89–103
5
Alkaline Earth Metals
titanium 47.867
40
barium 137.33
88
francium [223]
21
molybdenum 95.96
74
technetium [98]
75
ruthenium 101.07
76
W Re Os
tungsten 183.84
106
He helium 4.0026
Alkali Metals
rhenium 186.21
107
osmium 190.23
108
rhodium 102.91
77
Ir
iridium 192.22
109
palladium 106.42
78
silver 107.87
79
cadmium 112.41
80
indium 114.82
81
Pt Au Hg Tl
platinum 195.08
110
gold 196.97
111
mercury 200.59
112
thallium 204.38
113
tin 118.71
82
antimony 121.76
83
bromine 79.904
53
tellurium 127.60
84
I
iodine 126.90
85
Ne neon 20.180
Ar argon 39.948
36
Kr krypton 83.798
54
Xe xenon 131.29
86
Pb Bi Po At Rn lead 207.2
114
bismuth 208.98
115
polonium [209]
116
astatine [210]
117
radon [222]
118
Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv Uus Uuo
rutherfordium [261]
57
dubnium [262]
58
seaborgium [266]
59
bohrium [264]
60
hassium [277]
61
meitnerium [268]
darmstadtium roentgenium [271] [272]
copernicium [277]
62
63
65
64
ununtrium unknown
66
flerovium [289]
67
ununpentium unknown
livermorium [298]
ununseptium unknown
ununoctium unknown
68
69
70
71
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
lanthanum 138.91
89
cerium 140.12
90
praseodymium neodymium 140.91 144.24
91
Ac Th Pa
actinium [227]
thorium 232.04
protactinium 231.04
92
U
uranium 238.03
promethium [145]
93
samarium 150.36
94
europium 151.96
95
gadolinium 157.25
96
terbium 158.93
97
dysprosium 162.50
98
Np Pu Am Cm Bk Cf
neptunium [237]
plutonium [244]
americium [243]
curium [247]
berkelium [247]
californium [251]
holmium 164.93
99
erbium 167.26
100
thulium 168.93
101
ytterbium 173.05
102
lutetium 174.97
103
Es Fm Md No Lr
einsteinium [252]
fermium [257]
mendelevium [258]
nobelium [259]
lawrencium [262]
Use the larger periodic table on page 117 for reference.
Elements on the periodic table are organized into rows and columns. Each row is called a period. Every element in a row has the same number of atomic energy levels. For example, every element on the table’s top row has one energy level. As you move down the table, each row adds another energy level. Elements in the second row have two energy levels, while elements in the third row have three energy levels, and so on. The columns are called groups, or families. The groups are numbered from 1 to 18, left to right. Elements in the same group have similar chemical properties, but different physical properties.
CHEMISTRY CONNECTION Atoms in the same vertical column on the periodic table have the same number of electrons in the outermost energy level. These electrons are called valence electrons. Valence electrons interact with other atoms and give the atom many of its properties.
ATOMS, ELEMENTS, AND THE PERIODIC TABLE
17
The elements in group 2 are alkaline earth metals. These are shiny and silvery white in color. Other groups include noble gases (group 18), alkali metals (group 1), halogens (group 17), and transitional metals (groups 3 to 12).
CHEMISTRY CONNECTION Because an element can have different isotopes, the mass on the periodic table is actually the average atomic mass of the element. This number is calculated using a weighted average of all the masses of all the isotopes of an element.
18
CHEMISTRY | CHAPTER ONE
An element’s place on the periodic table can also give information about its electron configuration, or where the atom’s electrons are located in orbitals. Elements in the same column have the same valence electron configurations, which are the electrons in the atom’s outermost energy level. As a result, they behave in similar ways.
With this knowledge, chemists can predict how atoms will react in different situations. By using the periodic table, you can learn a lot about an element. For example, nitrogen (N) has an atomic number of 7. This number tells you that a neutral nitrogen atom has seven protons and seven electrons. Because nitrogen is in the second row or period of the table, its electrons can be found in two energy levels. You know that the first energy level contains two electrons. Putting it together, you can figure out that a nitrogen atom has two electrons in the first energy level and five electrons in the second energy level.
METALS, NONMETALS, AND METALLOIDS On the periodic table, there is a line that starts in front of the element boron (B) and steps down the table and ends between polonium (Po) and astatine (At). This line separates metals and nonmetals. Elements that are metals are located on the left of the line, while nonmetals are found on the right.
Some elements do not fit neatly into metal or nonmetal categories and have properties of both. These elements are called metalloids. They include boron, silicon, germanium, arsenic, antimony, tellurium, and polonium. On the periodic table, these elements are placed directly next to the dividing line between metals and nonmetals.
ISOTOPES OF AN ELEMENT In some cases, atoms of an element might be slightly different. They might weigh different amounts. How does this happen if all the atoms of an element have the same number of protons? Remember the neutrons in the atom’s nucleus? While the number of protons cannot change, atoms of the same element can have a different number of neutrons. When this happens, the atom’s atomic mass is changed. Atoms of the same element with different atomic masses are called isotopes.
ATOMS, ELEMENTS, AND THE PERIODIC TABLE
19
For example, the element lithium has three protons in its nucleus. These positively charged protons are separated and stabilized by either three or four neutrons. Depending on whether the atom has three or four neutrons, it will weigh different amounts. These two atoms—with either three or four neutrons—are isotopes of lithium.
VALENCE ELECTRONS AND THE OCTET RULE Hydrogen (H) and helium (He) are the exceptions to the octet rule. These two elements are perfectly happy with only two electrons in their outer energy levels.
Atoms like to be stable. Stability requires less energy. As with everything in the nature, atoms try to do the most work with the least amount of effort. A stable atom has a complete outer energy level. The electrons in the atom’s outer energy level are called valence electrons. The number of valence electrons determines the properties of the element. The octet rule in chemistry says that atoms are most stable when they have full outer energy levels, complete with eight electrons. Sometimes, an atom will have more or less than eight valence electrons. They will try to gain or lose valence electrons in order to reach their goal of eight. They can gain or lose electrons by bonding with other atoms, either of the same element or with different elements. KEY QUESTIONS • What are the main parts of an atom? What role does each part have? • Which elements do you come in contact with on a daily basis? What do you use them for? • Why is the periodic table useful? Would you group the elements in different ways?
20
CHEMISTRY | CHAPTER ONE
THREE-DIMENSIONAL ATOM Atoms can be broken down into three basic parts— protons, neutrons, and electrons. Using a few common household items, you can build three-dimensional models of different types of atoms.
• Label the sticker dots with symbols to represent the electrical charge. A plus symbol (+) represents a positive charge, a zero (0) is neutral, and a minus symbol (-) is a negative charge. • Select gumdrops to represent protons, neutrons, and electrons. Label each with the appropriate sticker dot. • Using the toothpicks, create a nucleus containing protons and neutrons for a lithium atom. You may need to break the toothpicks into pieces. Use the periodic table to figure out how many protons and neutrons are in a lithium atom.
Inquire & Investigate
Ideas for Supplies • small sticker dots • variety of different colored gumdrops • several wooden toothpicks • several long wooden skewers • periodic table (page 117)
• Attach electrons to your lithium atom’s nucleus. Use the long wooden skewers. • What charge does the atom have? Why? If you remove one electron, what charge does it now have? Why? • Using the periodic table, select several other atoms, such as helium, carbon, and oxygen. Create models for these atoms.
To investigate more, try combining several atom models to create molecules. Ideas include water (H2O) and carbon dioxide (CO2).
ATOMS, ELEMENTS, AND THE PERIODIC TABLE
21
Inquire & Investigate
VOCAB LAB Write down what you think each word means: electron, proton, neutron, orbital, valence electrons, element, metalloid, isotope, octet rule, and ion. Discuss your definitions with friends using reallife examples. Did you all come up with the same definitions? Turn to the text and the glossary if you need help.
USING THE PERIODIC TABLE The periodic table has several pieces of information about the atoms of the elements. In this activity, you will use the periodic table to investigate different elements.
Using a periodic table, answer the following questions. 1. What element has eight protons? 2. What is the atomic mass of magnesium? 3. How many electrons does an aluminum atom have? 4. What is the chemical symbol for silver? 5. How many elements are metalloids? How many are nonmetals? 6. What is the atomic number of iron? 7. How many protons, neutrons, and electrons does one atom of calcium have? 8. What is the atomic number of chromium? 9. Which element has an atomic mass of 65.38? 10. How many protons, neutrons, and electrons does the element sodium have?
To investigate more, select a few elements on the periodic table to research. How are they alike and how are they different? How does the periodic table give you information about the physical and chemical properties of these elements?
Check your answers in the resources at the end of this book. 22
CHEMISTRY | CHAPTER ONE
GLOSSARY acid rain: rain that is polluted by acid in the atmosphere and damages the environment.
acid: any material that can
accept a pair of electrons and has a pH less than 7.
of matter that cannot be broken down by chemical means. An atom is made up of a nucleus of protons and neutrons, surrounded by a cloud of electrons.
agriculture: growing plants and raising animals for food and other products.
atomic mass: the sum of
alcohol: any organic
atomic number: the number of protons in an atom’s nucleus.
compound in which a hydroxyl group (–OH) is bound to a saturated carbon atom.
alkaline: having a pH greater than 7.
allotropes: different structural forms of an element in which the atoms of the element are bonded together in a different way. alloy: a mixture of two or more metals, or of a metal and another element.
alpha decay: when a nucleus
breaks apart and emits a helium nucleus, called an alpha particle.
amu: a unit of measurement,
the number of protons and neutrons in an atom’s nucleus.
atomic symbol: the symbol that represents an element on the periodic table.
Avogadro’s law: a law that
states that the molar volumes of all ideal gases are the same.
base: a substance that
accepts a hydrogen ion (H+) from another substance. Examples include baking soda, ammonia, and oven cleaner.
basic: having a pH lower than 7. beta decay: a kind of
radioactive decay of an atomic nucleus when an electron called a beta particle is emitted.
atomic mass unit, used to measure the mass of atoms and molecules.
biochemistry: the study of
anion: an atom or group of
biology: the study of life
anode: the electrode
where oxidation occurs.
boiling point: the temperature at which a liquid boils.
aqueous solution: a solution
Boyle’s law: a gas law that
atoms with a negative charge.
in which the solvent is water.
atmosphere: a unit of measure of pressure.
110
atom: the smallest particle
CHEMISTRY | GLOSSARY
chemistry in living things.
and of living organisms.
states that the pressure and volume of a gas have an inverse relationship, when temperature is held constant.
carbon: an element found in all organic compounds. catalyst: a material that increases the rate of a chemical reaction without being consumed in the reaction. cathode: the electrode where reduction takes place. cation: an atom or group of atoms with a positive charge. cellular biology: the study of cell structure and function. characteristic: a feature of
a person, place, or thing, such as blue eyes or curly hair.
Charles’s law: a gas law that describes how gases expand when heated, and the relationship between volume and temperature. chemical equation: the use of symbols to represent a chemical reaction, with reactants on the left and products on the right. chemical reaction: a process where one or more substances are chemically charged and transformed into different substances. chemistry: the study of the properties of substances and how they react with one another. chromatography: a method of separating a mixture by passing it through a third material.
GLOSSARY coefficients: the numbers
placed before the reactants and products in a chemical equation so that the number of atoms in the products on the right side of the equation are equal to the number of atoms in the reactants on the left side.
combustion: a chemical reaction that produces heat and light.
composition: the ingredients in a mixture or substance. compound: a pure substance
made of two or more elements in specific proportions.
compress: to press or
squeeze something so that it fits into a smaller space.
concentration: the volume
crystal lattice: the structure in which ions or atoms are stacked in regular patterns to form a crystal.
electron: a negatively
data: information often given in the form of numbers.
element: a substance that
decomposition: a chemical reaction where larger molecules break into smaller molecules.
endothermic: a reaction that
density: the amount of
enzymes: catalysts in biochemical reactions.
matter in a give space, or mass divided by volume.
deposition: the process in which a gas directly becomes a solid, without becoming a liquid first.
dilution: the process of adding solvent to a solution to reduce its concentration of solute.
of an ingredient divided by the total volume of a mixture.
dissolve: to break up or be absorbed by a solvent.
condensation: the process in
distillation: the process
which a gas becomes a liquid.
conductivity: the ability
to allow electricity to flow through a substance.
conversion factor: a number used to multiply or divide a quantity when converting from one system of units to another.
covalent bond: a type of bond
that involves sharing a pair of electrons between atoms.
covalent compound: a
compound that is created when two or more atoms are held together using covalent bonds.
of heating a mixture of materials to separate them.
electrical charge: a property of matter. Protons have a positive charge and electrons have a negative charge.
electrochemistry: the
study of electricity and how it relates to chemical reactions.
electrode: the place where oxidation or deduction occurs in a voltaic cell. electrolyte: a compound that,
when dissolved in water, causes water to conduct electricity.
electron configuration:
a list of orbitals that hold an atom’s electrons.
charged particle that is found in orbitals outside the nucleus of an atom. cannot be broken down into simpler substances.
needs energy to take place.
equilibrium: the point
at which the products and the reactants of a chemical reaction have stabilized and the rates of forward and backward reactions are the same.
evaporation: the process in which a liquid becomes a gas. exothermic: a reaction that generates energy in the form of heat.
experimental error:
the difference between a measurement and the true value.
extract: to remove or take out by effort or force.
factor label method: a
way to convert units from one type to another using a conversion factor.
ferment: to go through a
chemical change that results in the creation of alcohol.
flame test: a test used to detect the presence of certain metal ions.
GLOSSARY
111
GLOSSARY flammable: easily burned. gamma radiation: the very
high energy electromagnetic radiation that is released when a nucleus undergoes radioactive decay.
gas: one of the three states
of matter. The particles of a gas are not bound to each other and move very fast in all directions. A gas does not have a definite shape or volume.
Gay-Lussac’s law: a gas law that states that the density of an ideal gas at constant pressure varies inversely with the gas’s temperature.
genetics: the study of how characteristics are passed from one generation to the next through genes.
geology: the scientific study
used to determine whether a solution is acidic or basic.
inhibitor: a material
that decreases the rate of a chemical reaction.
intermolecular force:
ideal gas: a gas that
follows all the rules of kinetic molecular theory.
CHEMISTRY | GLOSSARY
paper to test for acidity.
matter: any material or
units based on the metric system used by scientists.
ion: a particle with either a
positive or negative charge.
ionic bond: a type of bond
that transfers a valence electron from one atom to another.
ionic compound: a compound
formed when a cation and anion combine with each other.
kinetics: the study of
homogenous: something that is completely mixed with a uniform composition.
litmus: used with filter
international system of units (SI): a system of
graphite: a common black or gray mineral used as lead in pencils.
that is unevenly mixed.
matter. The particles of a liquid cluster together and flow. A liquid has a definite volume, but takes the shape of its container.
mass: the amount of material
isotope: an atom of an
heterogeneous: something
liquid: one of the three states of
a force that holds covalent molecules to one another.
of the history and physical nature of the earth.
half-life: the amount of time it takes for half of a reactant to be converted to product in a chemical or nuclear process.
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indicator: a compound
element that has a different number of neutrons.
chemical reaction rates.
kinetic energy: energy caused by an object’s motion. Le Chatelier’s principle:
a rule that states when the conditions of equilibrium change, the equilibrium shifts to minimize the effects of the changes.
limiting reactant: the
reactant that runs out first in a chemical reaction and determines the amount of products that can be formed.
that an object contains.
substance that takes up space.
melting point: the temperature at which a solid changes into a liquid. metabolism: chemical
reactions within living cells that are necessary for life.
metalloid: an element with properties of both metals and nonmetals.
metric system: a system of weights and measures based on the number 10.
mineral: a substance found in nature that is not an animal or a plant. mixture: a substance created by two or more substances that are combined physically but not chemically. molar mass: the weight of one mole of a substance. mole: a measurement of atoms
and molecules. One mole of a substance equals 6.02 x 1023 molecules of that substance.
GLOSSARY molecule: a group of atoms bonded together, the simplest structural unit of an element or compound. Molecules can break apart and form new ones, which is a chemical reaction. nanoparticle: a microscopic particle where size is measured in nanometers.
neutron: a particle in the
organic compound: a type of compound that contains the element carbon and often hydrogen, as well as other elements. organic: something that is or was living. organism: a living thing. oxidation: the loss of electrons
nucleus of an atom that does not have a charge.
or an increase in oxidation state by a molecule, atom, or ion.
nuclear emissions:
oxidizing agent: a
particles released during a nuclear reaction.
compound that causes another compound to be oxidized.
nuclear fission: a nuclear
particle: an extremely
reaction that releases energy when the nucleus of an atom splits into smaller pieces.
nuclear fusion: a nuclear
reaction in which the nuclei of two or more atoms collide at a very high speed and join to form a new nucleus.
nucleus: the center of an atom, which holds protons and neutrons.
octet rule: the way that
elements want to gain or lose electrons to have full outer energy levels of eight electrons.
orbit: the path an
electron follows around an atom’s nucleus.
orbitals: regions of space
outside the atom’s nucleus where electrons can be found.
ore: a naturally occurring
mineral that contains metal.
small piece of something.
pascal: a unit of
measurement of pressure.
percent yield calculation:
precipitate: a solid created from a chemical reaction in a solution. pressure: a force that pushes on something. product: the result of a chemical reaction. property: a characteristic quality or distinctive feature of something.
proton: a positively charged particle in the nucleus of an atom. radiation: small particles
released during the radioactive decay of an atom’s nucleus.
radioactive decay: when a nucleus spontaneously breaks apart and forms smaller particles.
a measurement of the accuracy of the result in a reaction, calculated by dividing the actual yield of a chemical reaction by the theoretical yield.
radioactive: something that undergoes radioactive decay.
periodic table: a chart that shows the chemical elements arranged according to their properties.
random error: a source of error in an experiment or chemical reaction that cannot be predicted or compensated for.
pH: a scale used to tell the acidity of a solution, with the value of 7 being neutral.
ratio: a comparison of two numbers or measurements, dividing one number by the other.
physics: the study of physical
forces, including matter, energy, and motion, and how these forces interact with each other.
radioisotope: any radioactive isotope.
reactant: an ingredient in a chemical reaction.
polyatomic ion: an ion that has more than one atom.
redox reaction: a reaction in which the oxidation state of the reactants changes.
potential energy: energy
reducing agent: a
that is stored.
compound that causes another to be reduced. GLOSSARY
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GLOSSARY scientific notation: a method that scientists use to write very large or very small numbers. significant figures: the
relate the masses or volumes of reactants and products in a chemical reaction to each other.
number of digits in a measured or calculated value that give meaningful information.
sublimation: the process in
simple displacement reaction: a reaction where
substance: the physical material from which something is made.
an element replaces another element in a compound.
solid: one of the three states
of matter. The particles of a solid are bound tightly. A solid has a definite shape and volume and does not flow.
which a solid becomes a gas without first becoming a liquid.
surface area: the total area of the surface of an object.
surface tension: the
tendency of liquids to keep a low surface area.
solubility: the property of
suspension: a
a substance to dissolve in a liquid called a solvent.
heterogeneous mixture that includes solid particles.
solute: the substance that
synthesis: the combination
is dissolved in a solution.
solution: a homogenous liquid mixture.
solvent: the substance that dissolves a solute. sphere: a round object,
such as a ball.
spontaneous: randomly. stabilize: to hold steady. states of matter: the form that matter takes. There are three common states of matter: solid, liquid, and gas.
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stoichiometry: a way to
CHEMISTRY | GLOSSARY
of smaller molecules to form larger ones.
theory: an unproven idea used to explain something. titration: using a neutralization reaction to find out the concentration of an acid or base.
Torr: a unit of pressure. valence electrons:
the number of s and p electrons beyond the most recent noble gas.
volume: a measure of how much space an object occupies.
Metric Conversions Use this chart to find the metric equivalents to the English measurements in this activity. If you need to know a half measurement, divide by two. If you need to know twice the measurement, multiply by two. How do you find a quarter measurement? How do you find three times the measurement? English
Metric
1 inch
2.5 centimeters
1 foot 1 yard 1 mile 1 pound 1 teaspoon 1 tablespoon
30.5 centimeters 0.9 meter 1.6 kilometers 0.5 kilogram 5 milliliters 15 milliliters
1 cup
237 milliliters
CHILDREN’S ACTIVITY/EDUCATION RESOURCE
focus on science
What makes up everything in the world around you? What exactly are the differences between solids, liquids, and gases? What causes two substances to react or change? Chemistry isn’t just a science in a lab, it’s everywhere. Chemistry: Investigate the Matter That Makes Up Your World introduces the fascinating world of protons, neutrons, and electrons. Learn how atoms and molecules combine to form ordinary objects, such as the chair you’re sitting on, the water in your glass, even you! • Investigative projects • Links to online resources • Graphic novel illustrations • Clear diagrams for visual learners AGES: 12–15 GUIDED READING LEVEL: Z
ALSO WRITTEN BY CARLA MOONEY The Brain: Journey Through the Universe Inside Your Head “ This short book is just plain fun to read. Its attractive, exciting, and colorful pages include a variety of cartoons that grab student attention and provide a humorous look at chapter topics. Many excellent examples and analogies are used to clarify concepts . . . . “ —National Science Teachers Association Forensics: Uncover the Science and Technology of Crime Scene Investigation 2013 Silver Moonbeam Award Winner
PRAISE FOR CHEMISTRY “ . . . a fantastic book and a great starting point to introduce young, budding scientists to the world of chemistry. The topics are explained very well and the experiments are easy for parents and their children to do together.” —Brandon S. Chance, M.S., CCHO Associate Director of Environmental Health and Safety, Office of Risk Management, Southern Methodist University 2013 Society of School Librarians: International Honor Book Award Winner