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Chapter 13. Chemical Bonding. Preview. CRCT Preparation. CRCT Preparation. Chapter 13. 1. How many electrons are in the second energy level of the atom shown? A 2 B 7 C 8 D 9. CRCT Preparation. Chapter 13. 1. How many electrons are in the second energy level of the atom shown? A 2

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slide1

Chapter 13

Chemical Bonding

Preview

CRCT Preparation

slide2

CRCT Preparation

Chapter 13

1. How many electrons are in the second energy level of the atom shown?

A2

B 7

C8

D9

slide3

CRCT Preparation

Chapter 13

1. How many electrons are in the second energy level of the atom shown?

A2

B 7

C 8

D9

slide4

CRCT Preparation

Chapter 13

2. Which of the following statements about helium atoms is true?

AHelium atoms can never have a full set of valence electrons.

BHelium atoms need only 2 valence electrons to have a full outermost energy level.

CHelium atoms do not have valence electrons.

DHelium atoms have the same number of valence electrons as sulfur atoms do.

slide5

CRCT Preparation

Chapter 13

2. Which of the following statements about helium atoms is true?

AHelium atoms can never have a full set of valence electrons.

B Helium atoms need only 2 valence electrons to have a full outermost energy level.

CHelium atoms do not have valence electrons.

DHelium atoms have the same number of valence electrons as sulfur atoms do.

slide6

CRCT Preparation

Chapter 13

3. Sodium chloride, or table salt, forms when a chlorine atom takes an electron from a neighboring sodium atom. Which of the following describes the force that holds sodium chloride together?

Aan ionic bond

Ba hydrogen bond

Ca metallic bond

Da covalent bond

slide7

CRCT Preparation

Chapter 13

3. Sodium chloride, or table salt, forms when a chlorine atom takes an electron from a neighboring sodium atom. Which of the following describes the force that holds sodium chloride together?

A an ionic bond

Ba hydrogen bond

Ca metallic bond

Da covalent bond

slide8

CRCT Preparation

Chapter 13

4. An aluminum ion has 13 protons, 14 neutrons, and 10 electrons. What is the charge of an aluminum ion?

A10 –

B3 –

C1 +

D3 +

slide9

CRCT Preparation

Chapter 13

4. An aluminum ion has 13 protons, 14 neutrons, and 10 electrons. What is the charge of an aluminum ion?

A10 –

B3 –

C1 +

D 3 +

slide10

CRCT Preparation

Chapter 13

5. What property of copper allows copper wire to bend without breaking?

ACopper atoms have 29 protons.

BCopper is found in Group 11 on the periodic table.

CCopper atoms do not have a full outermost energy level.

DCopper atoms form metallic bonds with each other.

slide11

CRCT Preparation

Chapter 13

5. What property of copper allows copper wire to bend without breaking?

ACopper atoms have 29 protons.

BCopper is found in Group 11 on the periodic table.

CCopper atoms do not have a full outermost energy level.

D Copper atoms form metallic bonds with each other.

slide12

CRCT Preparation

Chapter 13

6. According to the electron-dot diagram of oxygen shown, how many more valence electrons does the oxygen atom need to fill its outermost energy level?

A1

B2

C6

D8

slide13

CRCT Preparation

Chapter 13

6. According to the electron-dot diagram of oxygen shown, how many more valence electrons does the oxygen atom need to fill its outermost energy level?

A1

B 2

C6

D8

slide14

CRCT Preparation

Chapter 13

7. The ions that make up an ionic compound are bonded in a repeating three-dimensional pattern. What is this pattern called?

Achloride lattice

Bcovalent bond

Ccrystal lattice

Dcrystal pattern

slide15

CRCT Preparation

Chapter 13

7. The ions that make up an ionic compound are bonded in a repeating three-dimensional pattern. What is this pattern called?

Achloride lattice

Bcovalent bond

C crystal lattice

Dcrystal pattern

slide16

CRCT Preparation

Chapter 13

8. Which of the following forms when a neutral atom loses an electron?

Aa negative atom

Ba neutral ion

Ca positive ion

Da negative ion

slide17

CRCT Preparation

Chapter 13

8. Which of the following forms when a neutral atom loses an electron?

Aa negative atom

Ba neutral ion

C a positive ion

Da negative ion

slide18

CRCT Preparation

Chapter 13

9. During a laboratory experiment at Georgia State University, Juanita observes a model of two bonded atoms. She is told that the atoms are both nonmetals. Which of the following is a valid conclusion?

AShe is looking at a model of atoms held together by a covalent bond.

BShe is looking at a model of atoms held together by an ionic bond.

CShe is looking at a model of a metalloid.

DShe is looking at a model of a crystal lattice.

slide19

CRCT Preparation

Chapter 13

9. During a laboratory experiment at Georgia State University, Juanita observes a model of two bonded atoms. She is told that the atoms are both nonmetals. Which of the following is a valid conclusion?

A She is looking at a model of atoms held together by a covalent bond.

BShe is looking at a model of atoms held together by an ionic bond.

CShe is looking at a model of a metalloid.

DShe is looking at a model of a crystal lattice.

slide20

CRCT Preparation

Chapter 13

10. Which of an atom’s electrons are most likely to be involved in chemical bonding? Why?

slide21

CRCT Preparation

Chapter 13

10. Answer - Full-credit answers should include the following points:

• The valence electrons are most likely to be involved in chemical bonding.

• When two atoms are close to each other, the outermost electrons of one atom are closest to the nucleus of the other atom.

• The attraction between the outermost electrons in one atom and the positively-charged nucleus of the other atom contributes to the bond between the two atoms.

• The outermost electrons are shared, lost, or gained most easily.

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CRCT Preparation

Chapter 13

11. Why do atoms of the noble gases, in Group 18 on the periodic table, usually not form chemical bonds?

slide23

CRCT Preparation

Chapter 13

11. Answer - Full-credit answers should include the following points:

• The number of electrons in the outermost energy level of an atom determines whether an atom will form bonds.

• Atoms of the noble gases (Group 18) do not usually form chemical bonds because each atom has a full set of valence electrons.

• When the outermost energy level of an atom is full, the atom does not usually form bonds.