Deck 5: Chemical Bonding and Nomenclature

Question 1

The number of valence electrons in silicon is ________.

A) 2
B) 4
C) 6
D) 8

Answer 1

4

Question 2

The number of valence electrons in sulfur is ________.

A) 2
B) 4
C) 6
D) 8

Answer 2

6

Question 3

The number of valence electrons in aluminum is ________.

A) 2
B) 3
C) 5
D) 7

Answer 3

3

Question 4

The number of valence electrons in magnesium is ________.

A) 2
B) 4
C) 6
D) 8

Question 5

Which of the following elements has the lowest number of valence electrons?

A) magnesium
B) lithium
C) argon
D) phosphorus

Question 6

The number of valence electrons in nitrogen is ________.

A) 2
B) 3
C) 5
D) 6

Question 7

How many covalent bonds can a single oxygen atom form with other elements?

A) 3
B) 4
C) 2
D) 1

Question 8

Which phrase best describes a covalent bond between two atoms?

A) a stable arrangement of charged atoms held together by electrostatic forces
B) a stable arrangement of atoms made by sharing two electrons between adjacent atoms
C) uncommon, as electrons are free to jump from one atom to another
D) an exchange of nuclei between two atoms

Question 9

Which of the following represents the correct Lewis dot structure for selenium (Se)?

A)
B)
C)
D)

Question 10

Every single COVALENT bond represents ________ electrons.

A) one
B) two
C) four
D) One cannot say unless the atoms that make up the bond are known.

Question 11

Which of the following may not exist as a diatomic molecule?

A) oxygen
B) nitrogen
C) argon
D) hydrogen

Question 12

To follow the octet rule, how many electrons must a neutral sulfur atom gain when forming a negative ion?

A) 1
B) 2
C) 6
D) 8

Question 13

Which of the following elements has the highest number of valence electrons?

A) magnesium
B) lithium
C) argon
D) phosphorus

Question 14

Which of the following substances is molecular (composed of individual molecules) in composition?

A) carbon in coal
B) drinking water
C) a copper ingot
D) helium in a balloon

Question 15

How many valence electrons does a single, neutral iodine atom have?

A) 3
B) 4
C) 5
D) 7

Question 16

Which of the following exists as a diatomic molecule?

A) neon
B) oxygen
C) phosphorus
D) silicon

Question 17

Which of the following is considered an elemental substance?

A) I₂ (iodine)
B) H₂O (water)
C) Fe (an iron nail)
D) A and C are elemental substances.
E) All of the preceding are elemental substances.

Question 18

Which of the following statements best describes an ionic bond?

A) a strong lattice of positively and negatively charged atoms held together by electrical forces
B) the bonding type present in bound, non-metal atoms
C) the equal sharing of two electrons between adjacent atoms
D) the bonding type present between two metal atoms

Question 19

The number of valence electrons in neon is ________.

A) 2
B) 4
C) 6
D) 8

Question 20

How many covalent bonds can an element of Group VA form with other elements?

A) 4
B) 3
C) 2
D) 1

Question 21

Which of the following elements has the least number of valence electrons?

A) krypton
B) potassium
C) calcium
D) aluminum

Question 22

How many unpaired electrons does the oxide anion (O^₂-) have?

A) 3
B) 2
C) 1
D) 0

Question 23

The expected formula between potassium and sulfur is ________.

A) KS
B) K₂S₃
C) K₂S
D) KS₂

Question 24

Which of the following pairs has the same number valence electrons?

A) magnesium and potassium
B) lithium and calcium
C) argon and xenon
D) phosphorus and tellurium

Question 25

What is the most likely formula of the neutral, ionic compound formed by magnesium and oxygen?

A) Mg₂O
B) MgO₂
C) Mg₃O₂
D) MgO

Question 26

The expected formula between sodium and oxygen is ________.

A) NaO
B) Na₂O₂
C) Na₂O
D) Na₂O₃

Question 27

Methane has ________ covalent bonds and ________ lone pairs.

A) 4; 2
B) 4; 1
C) 4; 0
D) 2; 4

Question 28

What is the number of single bonds in C₂H₆O?

A) 5
B) 6
C) 7
D) 8

Question 29

The expected formula between aluminum and oxygen is ________.

A) AlO
B) AlO₂
C) AL₂O
D) AL₂O₃

Question 30

The expected formula between silicon and fluorine is ________.

A) SiF
B) SiF₂
C) SiF4
D) SiF6

Question 31

What is the most likely formula of the neutral, ionic compound formed by lithium and nitrogen?

A) LI₂N
B) LI₃N
C) LiN
D) LiN₂

Question 32

The expected formula between calcium and oxygen is ________.

A) CaO
B) CaO₂
C) Ca₂O
D) Ca₂O₅

Question 33

The expected formula between magnesium and sulfur is ________.

A) MgS
B) MgS₂
C) Mg₂S
D) Mg₂S₃

Question 34

The expected formula between calcium and iodine is ________.

A) CaI
B) CaL₂
C) Ca₂I
D) Ca₂I₃

Question 35

The expected formula between hydrogen and nitrogen is ________.

A) HN
B) NH₂
C) NH₃
D) NH₄

Question 36

The expected binary compound between magnesium and bromine is ________.

A) MgBr
B) MgBr₂
C) Mg₂Br
D) Mg₂Br₂

Question 37

Which of the following has the same number of valence electrons as sulfur?

A) nitrogen
B) oxygen
C) arsenic
D) boron

Question 38

Water has ________ covalent bonds and ________ lone pairs.

A) 2; 2
B) 2; 4
C) 2; 0
D) 2; 6

Question 39

Which of the following does not have the same number of valence electrons as the other three elements?

A) nitrogen
B) phosphorus
C) beryllium
D) arsenic

Question 40

How many valence electrons are needed to construct the Lewis dot structure of the BCL₃ molecule?

A) 11
B) 21
C) 24
D) 32

Question 41

The phosphate anion has ________ valence electrons.

A) 29
B) 30
C) 32
D) 36

Question 42

Nitrogen trifluoride has ________ bonds, ________ of which are single bonds.

A) 3; 3
B) 5; 1
C) 7; 2
D) 8; 3

Question 43

The number of valence electrons in the nitrate anion is ________.

A) 23
B) 24
C) 28
D) 30

Question 44

Which of the following has at least one double bond?

A) hydrogen
B) carbon dioxide
C) chlorine
D) nitrogen

Question 45

Hydrazine, N₂H₄, has ________ covalent bonds and ________ lone pairs.

A) 2; 2
B) 4; 2
C) 3; 4
D) 5; 2

Question 46

The number of valence electrons in the carbonate anion is ________.

A) 20
B) 22
C) 24
D) 26

Question 47

Each atom in the oxygen molecule contributes ________ valence electrons for a total of ________ electrons

A) 6; 12
B) 6; 8
C) 8; 6
D) 12; 6

Question 48

How many resonance structure could be drawn for the nitrate ion?

A) 0
B) 1
C) 2
D) 3

Question 49

Carbon tetrafluoride has ________ total valence electrons.

A) 24
B) 28
C) 32
D) 36

Question 50

Nitrogen trifluoride has ________ lone pairs of electrons.

A) 2
B) 5
C) 8
D) 10

Question 51

Nitrogen trifluoride has ________ valence electrons that are contributed by the nitrogen atom.

A) 5
B) 8
C) 10
D) 12

Question 52

Which of the following gases does not have a triple bond?

A) hydrogen cyanide
B) acetylene, C₂H₂
C) carbon dioxide
D) nitrogen

Question 53

The number of valence electrons that belong to the oxygens in the carbonate anion is ________.

A) 15
B) 18
C) 20
D) 24

Question 54

Which of the following has a triple bond?

A) water
B) carbon dioxide
C) oxygen
D) nitrogen

Question 55

Phosphine, PH₃, has ________ covalent pairs and ________ lone pairs.

A) 3; 0
B) 3; 1
C) 3; 2
D) 2; 0

Question 56

Which of the following has more than one double bond?

A) carbon monoxide
B) carbon dioxide
C) oxygen
D) nitrogen

Question 57

Hydrazine has ________ valence electrons.

A) 14
B) 12
C) 10
D) 8

Question 58

Nitrogen trifluoride has ________ valence electrons.

A) 20
B) 22
C) 24
D) 26

Question 59

Acetylene, C₂H₂, has ________.

A) two single bonds
B) two double bonds
C) one triple bond
D) both A and C

Question 60

Which of the following does not have at least one multiple covalent bond?

A) carbon dioxide
B) ethene, C₂H₄
C) hydrogen cyanide
D) ethane, C₂H₆

Question 61

Consider a bond A-B. If the difference in electronegativity is 3.5, the bond is considered ________.

A) ionic
B) covalent
C) polar covalent
D) hydrogen

Question 62

Identify the most electronegative element.

A) fluorine
B) oxygen
C) carbon
D) sodium

Question 63

Which of the following bonds will have the largest difference in electronegativity?

A) HBr
B) NaF
C) H₂
D) HS-

Question 64

The central atom in sulfuric acid is ________.

A) oxygen
B) sulfur
C) hydrogen
D) none of the above

Question 65

Identify the most polar covalent bond.

A) C-C
B) C-H
C) C-F
D) C-Cl

Question 66

Identify the least polar covalent bond.

A) C-C
B) C-H
C) C-F
D) C-Cl

Question 67

What is the chemical formula of calcium phosphate?

A) CaPO₄
B) Ca₂PO₄
C) Ca3PO₄
D) Ca3(PO₄)2

Question 68

Consider a bond A-B. If the difference in electronegativity is 0.0, the bond is considered ________.

A) ionic
B) covalent
C) polar covalent
D) hydrogen

Question 69

Identify the least electronegative element.

A) fluorine
B) oxygen
C) carbon
D) sodium

Question 70

If the electrons are shared equally between the two atoms, the bond is called ________.

A) ionic
B) non-polar covalent
C) hydrogen bonding
D) polar covalent

Question 71

Which of the following is the molecular formula for ozone?

A) O₃
B) O₃-
C) O₃-²
D) O₂-²

Question 72

Which of the following bonds will have the smallest difference in electronegativity?

A) HBr
B) NaF
C) H₂
D) HS-

Question 73

Which of the following compounds has a covalent bond?

A) NaCl
B) KBr
C) LiH
D) H₂

Question 74

What is the chemical name of the compound whose formula is K₂O?

A) dipotassium oxygen
B) potassium oxide
C) potasside oxygen
D) potassium oxygen

Question 75

Consider a bond A-B. If the difference in electronegativity is 1.0, the bond is considered ________.

A) ionic
B) covalent
C) polar covalent
D) hydrogen

Question 76

In a(n) ________ bond, the electrons are transferred.

A) ionic
B) covalent
C) hydrogen bonding
D) polar covalent

Question 77

Which of the following phrases best describes the H-O bonds present in water (H₂O)?

A) nonpolar and ionic
B) nonpolar and covalent
C) polar and ionic
D) polar and covalent

Question 78

Identify the ionic bond.

A) C-S
B) Na-F
C) N-O
D) F-F

Question 79

The numerical rating of an atom's ability to attract the shared electrons is called ________.

A) electronegativity
B) ionization
C) covalency
D) redistribution

Question 80

In a(n) ________ bond, the electrons are shared unequally.

A) ionic
B) non-polar covalent
C) hydrogen bonding
D) polar covalent