1. Table of Contents Chapter Preview
5.1 Atoms, Bonding, and the Periodic Table
5.2 Ionic Bonds
5.3 Covalent Bonds
5.4 Bonding in Metals

2. Chapter Preview Questions
1. The atom is made of protons, electrons, and
a. valence electrons.
b. neutrons.
c. molecules.
d. ions.

3. Chapter Preview Questions
1. The atom is made of protons, electrons, and
a. valence electrons.
b. neutrons.
c. molecules.
d. ions.

4. Chapter Preview Questions
2. Reactant atoms and molecules interact to form products with
a. identical physical properties.
b. different physical properties.
c. identical chemical properties.
d. different chemical properties.

5. Chapter Preview Questions
2. Reactant atoms and molecules interact to form products with
a. identical physical properties.
b. different physical properties.
c. identical chemical properties.
d. different chemical properties.

6. Chapter Preview Questions
3. In chemical reactions, the number of atoms
a. varies according to the elements involved.
b. changes from one reactant to another.
c. stays the same.
d. depends on atom arrangement.

7. Chapter Preview Questions
3. In chemical reactions, the number of atoms
a. varies according to the elements involved.
b. changes from one reactant to another.
c. stays the same.
d. depends on atom arrangement.

8. Chapter Preview Questions
4. Compounds are formed by
a. combining two or more different elements.
b. bombarding atoms with high-speed particles.
c. combining two or more different nuclei.
d. dissolving a solid in a liquid.

9. Chapter Preview Questions
4. Compounds are formed by
a. combining two or more different elements.
b. bombarding atoms with high-speed particles.
c. combining two or more different nuclei.
d. dissolving a solid in a liquid.

10. Section 1: Atoms, Bonding, and the Periodic Table
Standard 8.3.f: Students know how to use the periodic table to identify elements in simple compounds.

11. Valence Electrons and Bonding
How is the reactivity of elements related to valence electrons in atoms? Valence electrons
The number of valence electrons in an atom of an element determines the ways in which the atom can bond with other atoms.
Electrons in the outermost shell of an atom.
Have the highest energy level.
Involved in bonding between atoms.

12. Valence Electrons and Bonding
Electron Dot Diagrams
Include the symbol for an element surrounded by dots that represent the number of valence electrons.

13. Valence Electrons and Bonding
Chemical Bond The Rule of 8
The force of attraction that holds two atoms together as a result of the rearrangement of electrons between them.
Electrons may be transferred from one atom to another, or they may be shared between the atoms.
Atoms are unlikely to react when they have 8 valence electrons.

14. How the Periodic Table Works
What does the periodic table tell you about the atoms of the elements?
The periodic table reveals the underlying atomic structure of atoms, including the arrangement of the electrons.

15. How the Periodic Table Works
The number of valence electrons varies by group. Group 3 through 12 elements do not follow the same pattern as the other groups!
Group 1 elements have 1 valence electron.
Group 2 elements have 2 valence electrons.
Groups 3 – 12 have 1 to 2 valence electrons.
Group 13 elements have 3 valence electrons.
Groups 14 – 18 have 4, 5, 6, 7, and 8 valence electrons, respectively.

16. Example of Group 1 elements
Lithium Atom: 3 Protons/3 Neutrons 3 Electrons – 1 in Valence Shell
Sodium Atom: 11 Protons/11 Neutrons 11 Electrons – 1 in Valence Shell

17. The electrons involved in bonding between atoms are
Section 1 Quick Quiz
The electrons involved in bonding between atoms are
inside the nucleus.
closest to the nucleus.
positively charged.
valence electrons.
Answer:
D – Valence electrons

18. How many valence electrons do Group 13 elements have?
Section 1 Quick Quiz
How many valence electrons do Group 13 elements have? 5 8 3 6
Answer:
C – 3 Valence Electrons

19. What is the greatest number of valence electrons an atom can have?
Section 1 Quick Quiz
What is the greatest number of valence electrons an atom can have? 5 8 3 6
Answer:
B – 8 Valence Electrons

20. Which Group of elements is the least reactive?
Section 1 Quick Quiz
Which Group of elements is the least reactive?
Group 1
Group 2
Group 17
Group 18
Answer:
D – Group 18

21. Section 1 Quick Quiz
Each family in the periodic table has its own characteristic properties based on the number of
valence electrons
neutrons
protons
ions
Answer:
A – Valence electrons

22. Section 1 Quick Quiz
If atoms of a halogen nonmetal (Group 17) gain one electron, the atoms then have
no valence electrons.
7 valence electrons.
8 valence electrons.
17 valence electrons.
Answer:
C – 8 valence electrons

23. Section 2: Ionic Bonds
Standard 8.3.b: Students know that compounds are formed by combining two or more different elements and that compounds have properties that are different from their constituent elements.
Standard 8.3.c: Students know that atoms and molecules form solids by building up repeating patterns, such as the crystal structure of NaCl or long-chain polymers.

24. Ions What is an ion? How do ions form bonds?
An ion is an atom or group of atoms that has an electric charge.
When an atom loses an electron it becomes a positive ion.
When an atom gains an electron it becomes a negative ion.
Ionic bonds form as a result of the attraction between positive and negative ions.

25. Ionic Compounds Sodium has 1 valence electron
Chlorine has 7 valence electrons

26. Chemical Formulas and Names
How are the formulas and names of ionic compounds written?
Positive Negative
Ion Ion -
NaCl
When ionic compounds form, the ions come together in a way that balances out the charges on the ions. The chemical formula for the compound reflects this balance.
For an ionic compound, the name of the positive ion comes first, followed by the name of the negative ion.

27. Chemical Formulas and Names
What is a chemical formula? What is a subscript? Chemical Formula
It is a combination of symbols that shows the ratio of elements in a compound.
A subscript tells you the ratio of elements in the compound.
CO Subscript
The ratio of Carbon to Oxygen is 1 to 2.

28. Properties of Ionic Compounds
What are the properties of ionic compounds?
In general, ionic compounds are hard, brittle solids with high melting points.
When melted or dissolved in water, they conduct electric current.

29. When an atom loses an electron, it becomes a
Section 2 Quick Quiz
When an atom loses an electron, it becomes a
positive ion.
negative ion.
neutral ion.
neutral atom.
Answer:
A – positive ion

30. An ionic bond is an attraction between
Section 2 Quick Quiz
An ionic bond is an attraction between
similarly charged ions.
oppositely charged ions.
neutral ions.
neutral atoms.
Answer:
B – oppositely charged ions

31. Ionic compounds are electrically
Section 2 Quick Quiz
Ionic compounds are electrically
charged
positive
neutral
negative
Answer:
C – neutral

32. In what form can an ionic compound conduct electricity?
Section 2 Quick Quiz
In what form can an ionic compound conduct electricity?
as a solid
when dissolved in water
as a crystal
when warmed slightly
Answer:
B – when dissolved in water

33. C – They form hard, brittle crystals with characteristic shapes
Section 2 Quick Quiz
Which of the following is a characteristic property of ionic compounds?
They have low melting points.
They have low boiling points.
They form hard, brittle crystals with characteristic shapes.
They contain no charged particles.
Answer:
C – They form hard, brittle crystals with characteristic shapes

34. Section 2 Quick Quiz
In the chemical formula for an ionic compound, which item is written first?
positive ion
negative ion
subscript
charge
Answer:
A – positive ion

35. Section 3: Covalent Bonds
Standard 8.3.b: Students know that compounds are formed by combining two or more different elements and that compounds have properties that are different from their constituent elements.
Standard 8.7.c: Students know substances can be classified by their properties, including their melting temperature, density, hardness, and thermal and electrical conductivity.

36. How Covalent Bonds Form
What holds covalently bonded atoms together?
The force that holds atoms together in a covalent bond is the attraction of each atom’s nucleus for the shared pair of electrons.

37. How Covalent Bonds Form
Double and triple bonds can form when atoms share more than one pair of electrons.
How do double and triple bonds form?

38. How Covalent Bonds Form
A carbon dioxide molecule has two double bonds.

39. How Covalent Bonds Form
A nitrogen molecule is an example of a triple bond

40. Molecular Compounds What are the properties of molecular compounds?
Molecular compounds generally have lower melting points and boiling points than ionic compounds.
They do not conduct electric current when melted or dissolved in water.

41. Unequal Sharing of Electrons
How does unequal sharing of electrons affect molecules? Polar bond Nonpolar bond
Unequal sharing of electrons causes the bonded atoms to have slight electrical charges. A covalent bond in which electrons are shared unequally. A covalent bond in which electrons are shared equally.

42. Unequal Sharing of Electrons
Fluorine forms a nonpolar bond with another fluorine atom.

43. Unequal Sharing of Electrons
In hydrogen fluoride, fluorine attracts electrons more strongly than hydrogen does, so the bond formed is polar.

44. Unequal Sharing of Electrons
A carbon dioxide molecule is a nonpolar molecule because of its straight-line shape.

45. Unequal Sharing of Electrons
In contrast, a water molecule is a polar molecule because of its bent shape.

46. Water Molecule – Polar Bonding

47. A chemical bond formed when two atoms share electrons is called a(n)
Section 3 Quick Quiz
A chemical bond formed when two atoms share electrons is called a(n)
ionic bond
covalent bond
polyatomic bond
crystal bond
Answer:
B – covalent bond

48. C – two pairs of electrons shared between two atoms
Section 3 Quick Quiz
What is a double bond?
a bond between two atoms
one pair of electrons shared between two atoms
two pairs of electrons shared between two atoms
two pairs of electrons shared between four atoms
Answer:
C – two pairs of electrons shared between two atoms

49. A covalent bond in which electrons are shared unequally is
Section 3 Quick Quiz
A covalent bond in which electrons are shared unequally is
polar.
a double bond.
ionic.
polyatomic.
Answer:
A – polar

50. D – The liquids do not mix
Section 3 Quick Quiz
Water is polar and oil in nonpolar. What happens when the two liquids are poured into the same container?
Both liquids become nonpolar.
A gas is produced.
The liquids mix well.
The liquids do not mix.
Answer:
D – The liquids do not mix

51. Section 4: Bonding in Metals
Standard 8.7.c: Students know substances can be classified by their properties, including their melting temperature, density, hardness, and thermal and electrical conductivity.

52. Metals and Alloys
How do the properties of metals and alloys compare? Alloy
Alloys are generally stronger and less reactive than the pure metals from which they are made. A mixture of two or more elements, at least one of which is a metal. Example: Stainless steel – an alloy of iron, carbon, nickel, and chromium.

53. Metallic Bonding How do metal atoms combine? What is a metallic bond?
Metal atoms combine in regular patterns in which the valence electrons are free to move from atom to atom. An attraction between a positive metal ion and the electrons around it

54. Metallic Properties
How does metallic bonding result in useful properties of metals? malleable ductile
The “sea of electrons” model of solid metals explains their ability to conduct heat and electricity, the ease with which they can be made to change shape, and their luster. Able to be rolled into thin sheets or beaten into complex shapes Able to be bent easily and pulled into thin strands or wires

55. Section 4 Quick Quiz
A mixture that is made of two or more elements-one that is a metal-that has the properties of metal is a(n)
polymer
monomer
alloy
ceramic
Answer:
C – alloy

56. Steel is an alloy of one or more elements combined with
Section 4 Quick Quiz
Steel is an alloy of one or more elements combined with
copper
gold
iron
lead
Answer:
C – iron

57. Brass and steel are examples of
Section 4 Quick Quiz
Brass and steel are examples of
alloys
elements
pure metals
valence electrons
Answer:
A – alloys

58. Section 4 Quick Quiz
Which of the following terms means that metals can be rolled into thin sheets, as in aluminum foil, or beaten into complex shapes?
polar
alloy
ductile
malleable
Answer:
D – malleable

59. Section 4 Quick Quiz
Which of the following terms means that metals can be pulled into thin strands or wires?
polar
alloy
ductile
malleable
Answer:
C – ductile