1. Chemical Bonding
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2. Lesson 1 Reading Guide - KC
Electrons and Energy Levels
How is an electron’s energy related to its distance from the nucleus?
Why do atoms gain, lose, or share electrons?
Lesson 1 Reading Guide - KC

3. The Periodic Table
Elements on the periodic table are organized in periods (rows) and groups (columns).
The periodic table lists elements in order of atomic number, which increases from left to right as you move across a period.
Lesson 1-1

4. The three main regions of elements on the periodic table classify elements as metals, nonmetals, or metalloids.
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5. The Periodic Table (cont.)
Except for hydrogen, elements on the left side of the table are metals.
Nonmetals are on the right side of the table.
Metalloids form the narrow stair-step region between metals and nonmetals.
Lesson 1-1

6. Atoms Bond
A chemical bond is a force that holds two or more atoms together in a compound.
Atoms contain protons, neutrons, and electrons.
Each proton has a positive charge; each neutron has no charge; and each electron has a negative charge.
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7. Protons and neutrons are in an atom’s nucleus
Protons and neutrons are in an atom’s nucleus. Electrons move around the nucleus.
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8. Atoms Bond (cont.)
The atomic number of an element is the number of protons in each atom of that element.
An electron moves around the nucleus at a distance that corresponds to its amount of energy.
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9. Atoms Bond (cont.)
Areas of space in which electrons move around the nucleus are called energy levels.
Electrons closest to the nucleus have the least amount of energy. Electrons farthest from the nucleus have the greatest amount of energy.
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10. Electron Energy Levels
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11. Atoms Bond (cont.)
The attraction between the positive nucleus of one atom and the negative electrons of another atom is what creates a chemical bond.
A valence electron is an outermost electron of an atom that participates in chemical bonding.
Lesson 1-2

12. Atoms Bond (cont.) valence
from Latin valentia, means “strength, capacity”
The number of valence electrons in each atom of an element can help determine the type and number of bonds that an atom can form.
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13. Valence electrons can be found by looking at the group an element is in on the periodic table.
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14. Atoms Bond (cont.)
In 1916 an American chemist named Gilbert Lewis developed the electron dot diagram, a model that represents valence electrons in an atom as dots around the element’s chemical symbol.
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15. Lesson 1-3

16. Atoms Bond (cont.)
Atoms with eight valence electrons are chemically stable and do not easily react with other atoms.
Atoms that have between one and seven valence electrons are reactive or chemically unstable and easily bond with other atoms to form chemically stable compounds.
Lesson 1-2

17. Atoms Bond (cont.) The elements in group 18 are called noble gases.
With the exception of helium, noble gases have eight valence electrons and are chemically stable.
Lesson 1-2

18. Atoms gain, lose, or share valence electrons and become chemically stable.
Lesson 1-2

19. Lesson 2 Reading Guide - KC
Compounds, Chemical Formulas, and Covalent Bonds
How do elements differ from the compounds they form?
What are some common properties of a covalent compound?
Lesson 2 Reading Guide - KC

20. Lesson 2 Reading Guide - Vocab
Compounds, Chemical Formulas, and Covalent Bonds
covalent bond
molecule
polar molecule
chemical formula
Lesson 2 Reading Guide - Vocab

21. From Elements to Compounds
Compounds are chemical combinations of different types of atoms.
Chemical bonds join atoms together.
Lesson 2-1

22. From Elements to Compounds (cont.)
bond
Science Use a force that holds atoms together in a compound
Common Use a close personal relationship between two people
Lesson 2-1

23. Covalent Bonds—Electron Sharing
A covalent bond is a chemical bond formed when two atoms share one or more pairs of valence electrons.
A compound formed from many covalent bonds is called a covalent compound.
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24. Atoms with less than eight valence electrons become chemically stable by forming a chemical bond.
Lesson 2-2

25. Covalent Bonds—Electron Sharing (cont.)
A single covalent bond exists when two atoms share one pair of valence electrons.
A double covalent bond exists when two atoms share two pairs of valence electrons
A triple covalent bond exists when two atoms share three pairs of valence electrons.
Lesson 2-2

26. The more valence electrons that two atoms share, the stronger the covalent bond is between the atoms.
Lesson 2-2

27. Covalent Compounds (cont.)
A molecule is a group of atoms held together by covalent bonding that acts as an independent unit.
A molecule that has a partial positive end and a partial negative end because of unequal sharing of electrons is a polar molecule.
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28. Atoms of a polar molecule share their valence electrons unequally.
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29. Atoms of a nonpolar molecule share their valence electrons equally.
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30. Covalent Compounds (cont.)
A chemical formula is a group of chemical symbols and numbers that represent the elements and the number of atoms of each element that make up a compound.
A chemical formula describes the types of atoms in a compound or a molecule, but it does not explain the shape or appearance of the molecule.
Lesson 2-3

31. Chemical formulas and molecular models provide information about molecules.
Lesson 2-4

32. Lesson 3 Reading Guide - KC
Ionic and Metallic Bonds
What is an ionic compound?
How do metallic bonds differ from covalent and ionic bonds?
Lesson 3 Reading Guide - KC

33. Understanding Ions
An ion is an atom that is no longer electrically neutral because it has lost or gained valence electrons.
ion
from Greek ienai, means “to go”
Lesson 3-1

34. Understanding Ions (cont.)
Because electrons have a negative charge, losing or gaining an electron changes the overall charge of an atom.
Atoms that lose valence electrons become ions with a positive charge.
Metal atoms, such as sodium, become more stable when they lose valence electrons and form a chemical bond with a nonmetal.
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35. Sodium atoms have a tendency to lose a valence electron
Sodium atoms have a tendency to lose a valence electron. Chlorine atoms have a tendency to gain a valence electron.
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36. Understanding Ions (cont.)
Atoms are electrically neutral because they have the same number of protons and electrons.
Once an atom gains or loses electrons, it becomes a charged ion.
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37. Ionic Bonds—Electron Transferring
When forming a compound, the nonmetal atoms gain the electrons lost by the metal atoms.
The attraction between positively and negatively charged ions in an ionic compound is an ionic bond.
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38. An ionic bond forms between Na and Cl when an Na atom transfers an electron to a Cl atom.
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39. Ionic Compounds
Individual ions in an ionic compound are strongly attracted to each other.
Covalent compounds are made up of many molecules.
When nonmetal ions bond to metal ions in an ionic compound there is a large collection of oppositely charged ions and no molecules.
Lesson 3-3

40. Metallic Bonds—Electron Pooling
A metallic bond is a bond formed when many metal atoms share their pooled valence electrons.
Valence electrons in metals are not bonded to one atom.
Instead, a “sea of electrons” surrounds the positive ions.
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41. Valence electrons are free to move among all the aluminum (Al) ions.
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42. Metallic Bonds—Electron Pooling (cont.)
Metals are good conductors of thermal energy and electricity.
Metals are shiny because the valence electrons at the surface of a metal interact with light.
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43. Lesson 3-4

44. Lesson 3-4