Test 2 Quiz Questions

Question 1

In what directions on the periodic table does electronegativity tend to increase? (choose all that apply)

Options:
1) Going down a group
2) Going to the right in a period
3) Going to the left in a period
4) Going up a group

Answer 1

2) Going to the right in a period
4) Going up a group

Question 2

Based on their position on the periodic table, which bond do you expect to be the most polar

Options:
1) Al - S
2) P - Cl
3) Be - Cl
4) Al - P

Answer 2

3) Be - Cl

Question 3

When many atoms combine to form ionic compounds, the reaction is highly exothermic. Where is most of this energy coming from?

Options:
1) The energy released when the ions combine to form the ionic compounds

2) The energy associated with formation of the cations

3) The energy associated with forming both the anion and the cation

4) The energy released when atoms gain electrons to make the anions

Answer 3

1) The energy released when the ions combine to form the ionic compounds.

Question 4

Is each of the following steps for the formation of magnesium chloride endothermic or exothermic

1) Vaporization of magnesium
2) Ionization of magnesium
3) Dissociation of chlorine
4) Chlorine gaining electrons to form the chloride ion
5) Magnesium and chloride ions combining to form the solid salt

Answer 4

1) Endothermic
2) Endothermic
3) Endothermic
4) Exothermic
5) Exothermic

Question 5

When many atoms combine to form ionic compounds the reaction is highly exothermic. Where is most of this energy coming from?

Options:
1) The energy released when atoms gain electrons to make the anions

2) The energy associated with formation of the cations

3) The energy associated with forming both the anion and the cation

4) The energy released when the ions combine to form the ionic compounds

Answer 5

4) The energy released when the ions combine to form the ionic compounds

Question 6

Why is the lattice energy of LiF expected to be greater than the lattice energy than NaF?

Options:
1) The lithium ion has a larger charge than the sodium ion.

2) The lithium ion is larger than the sodium ion.

3) The lithium ion is smaller than the sodium ion

4) The lithium ion has a smaller charge than the sodium ion.

Answer 6

3) The lithium ion is smaller than the sodium ion

Question 7

Formal way to write Barium Chloride

Answer 7

BaCl2

Question 8

Formal way to write Lithium Fluoride

Answer 8

LiF

Question 9

Formal way to write Lead(II) Oxide

Answer 9

PbO

Question 10

Formal way to write Silver Sulfide

Answer 10

Ag2S

Question 11

What roman numeral is required in the name of the following compound? Pb(SO3)2

Options:
1) No roman numeral is required.
2) III
3) II
4) I
5) IV

Answer 11

5) IV

Question 12

What roman numeral is required in the name of the following compound? Ag2SO4

Options:
1) III
2) IV
3) No roman numeral is required.
4) I
5) II

Answer 12

3) No roman numeral is required.

Question 13

Formal way to write Potassium Bicarbonate (potassium hydrogen carbonate)

Answer 13

KHCO3

Question 14

Formal way to write Calcium Bicarbonate (calcium hydrogen carbonate)

Answer 14

Ca(HCO3)2

Question 15

Formal way to write Lead (II) Carbonate

Answer 15

PbCO3

Question 16

Formal way to write Lead (IV) Hydroxide

Answer 16

Pb(OH)4

Question 17

Spell out N2O4

Answer 17

Dinitrogen Tetroxide

Question 18

Spell out PCl5

Answer 18

Phosphorus Pentachloride

Question 19

Formal way to write Carbon Tetrabromide

Answer 19

CBr4

Question 20

Formal way to write Xenon tetroxide

Answer 20

XeO4

Question 21

True or False
F has a greater electronegativity than Kr

Answer 21

True

Question 22

True or False
Cl has a smaller electronegativity than Br

Answer 22

False

Question 23

True or False
C has a greater electronegativity than N

Answer 23

False

Question 24

Draw the dot diagram of ClO3- that minimizes formal charge. (each atom is bound to the central chlorine)

The diagram has how many single, double and non-bonding pairs on the Cl

Answer 24

1 single bond
2 double bonds
1 non-bonding pair on Cl

Question 25

Draw the dot diagram of SOCl2 that minimizes formal charge. (each atom is bound to the central sulfur) The diagram has how many single, double and non-bonding pairs on the S

Answer 25

2 single bonds 1 double bond 1 non-bonding pair on S

Question 26

Draw the dot diagram of NO2+ that minimizes formal charge. The diagram has how many single, double and non-bonding pairs on the N

Answer 26

0 single bonds 2 double bonds 0 non-bonding pairs on N

Question 27

Which of the following elements can form compounds with an expanded octet? Options: 1) None of the above can 2) F 3) Be 4) N 5) Br

Answer 27

5) Br

Question 28

Which of the following elements can form compounds with an expanded octet? Options: 1) C 2) None of the above 3) F 4) P 5) N

Answer 28

4) P

Question 29

Which of the following elements can form compounds with an expanded octet? Options: 1) Li 2) Se 3) All of the above 4) C 5) F

Answer 29

2) Se

Question 30

How many electrons are found around the following atoms when they are in a molecule and have less than an octet? ( a number will be used more than once) H- Be- B- Al- Options: 1 2 4 6 8 7

Answer 30

H- 2 Be- 4 B- 6 Al- 6

Question 31

Match the number of electron domains to the domain geometry 1) Two domains- 2) Three domains- 3) Four domains- 4) Five domains- 5) Six domains- Options: Octahedral Linear Tetrahedral Trigonal bipyramidal Trigonal planar

Answer 31

1) Linear 2) Trigonal planar 3) Tetrahedral 4) Trigonal bipyramidal 5) Octahedral

Question 32

What is the electron domain geometry around the middle oxygen in ozone - O3? Options: 1) linear 2) tetrahedral 3) trigonal bipyramidal 4) octahedral 5) trigonal planar

Answer 32

5) trigonal planar

Question 33

What is the electron domain geometry around nitrogen in NH3? Options: 1) linear 2) trigonal planar 3) octahedral 4) tetrahedral 5) trigonal bipyramidal

Answer 33

4) tetrahedral

Question 34

Give the approximate bond angle(s) for a central atom with an octahedral electron domain geometry. Options: 1) 120° 2) 90 & 120 3) 109.5 4) 90° 5) 180°

Answer 34

4) 90°

Question 35

Give the approximate bond angle(s) for a central atom with a linear electron domain geometry. Options: 1) 90 2) 120° 3) 109.5° 4) 180° 5) 90° & 120

Answer 35

4) 180°

Question 36

Give the approximate bond angle(s) for a central atom with a trigonal bipyramidal electron domain geometry. Options: 1) 90° & 120 2) 180° 3) 90 4) 109.5 5) 120°

Answer 36

1) 90° & 120

Question 37

Indicate whether each of the molecules below is polar or not polar. 1) CO2 2) CH2O 3) SF6 4) HCN

Answer 37

1) Not polar 2) Polar 3) Not polar 4) Polar

Question 38

Indicate whether each of the molecules below is polar or not polar 1) SeF4 2) CS2 3) SCO 4) H2O

Answer 38

1) Polar 2) Not polar 3) Polar 4) Polar

Question 39

Indicate whether each of the molecules below is polar or not polar 1) CH4 2) N2 3) PF5 4) CH3F

Answer 39

1) Not polar 2) Not polar 3) Not polar 4) Polar

Question 40

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N2O NCl3 NO2-

Answer 40

1) N2O 2) NO2- 3) NCl3

Question 41

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. CF4 CS2 SCl2

Answer 41

1) CS2 2) CF4 3) SCl2