Deck 4: Chemical Bonds

Question 1

Which of the following pairs is isoelectronic?

A) Ar and Ne
B) Ar and Na⁺
C) Ar and F^-
D) Ar and S^2-

Answer 1

Ar and S^2-

Question 2

The number of protons in a sodium ion, Na⁺, is

A) 10.
B) 11.
C) 12.
D) 23.

Answer 2

11.

Question 3

All of the following pairs are isoelectronic EXCEPT

A) Ne and Rn.
B) Rb⁺ and Sr²⁺.
C) Ne and Mg²⁺.
D) F^- and Ne.

Answer 3

Ne and Rn.

Question 4

A sodium ion, Na⁺, has the same electron configuration as a(n)

A) sodium atom.
B) chlorine atom.
C) neon atom.
D) argon atom.

Question 5

Which molecule is NOT likely to exist?

A) N₂
B) Br₂
C) CI₄
D) Ar₂

Question 6

The number of protons in a chloride ion, Cl^-, is

A) 16.
B) 17.
C) 18.
D) 35.

Question 7

Mg²⁺ has the same electronic structure as

A) Ne.
B) Mg.
C) C.
D) Ar.

Question 8

When barium reacts with iodine, barium ions, Ba²⁺, and iodide ions, I^-, are formed. In this reaction, iodine atoms

A) lose electrons.
B) gain electrons.
C) lose protons.
D) gain protons.

Question 9

A chloride ion, Cl^- has the same electron configuration as a(n)

A) sodium atom.
B) chlorine atom.
C) neon atom.
D) argon atom.

Question 10

The inertness of the noble gases is due to

A) the outermost shell has six electrons.
B) the number of protons and neutrons.
C) the bonds they form with other elements.
D) the outermost shell has an octet of electrons, except for helium which has two electrons.

Question 11

Which of the following molecules is NOT likely to exist?

A) CO₂
B) HCl
C) CCl₄
D) RnH

Question 12

All of the following species are isoelectronic to Mg²⁺ EXCEPT

A) Li⁺.
B) Na⁺.
C) Ne.
D) O^2-.

Question 13

The number of electrons in a sodium ion, Na⁺, is

A) 10.
B) 11.
C) 12.
D) 23.

Question 14

When calcium reacts with iodine, calcium ions, Ca²⁺, and iodide ions, I^-, are formed. In this reaction, calcium atoms

A) lose electrons.
B) gain electrons.
C) lose protons.
D) gain protons.

Question 15

The nature of bonding forces in matter influences which of the following observable properties of the matter?

A) the optical property
B) the state of the matter at room temperature
C) the strength and rigidity
D) all of the above

Question 16

The number of electrons in a chloride ion, Cl^-, is

A) 16.
B) 17.
C) 18.
D) 35.

Question 17

The number of electrons in a sulfide ion, S^2-, is

A) 16.
B) 14.
C) 18.
D) 32.

Question 18

The noble gases are inert. This means they

A) undergo very few chemical reactions.
B) exist as gases at room temperature.
C) undergo many chemical reactions.
D) lose and gain electrons easily.

Question 19

Noble gases are unreactive because of their electronic structures. The kind of reasoning that states "if other elements could be made to achieve noble gas electronic structures they would be more stable" is called

A) logic.
B) inductive reasoning.
C) deductive reasoning.
D) critical thinking.

Question 20

When atoms lose or gain electrons in chemical reactions they form

A) new atoms.
B) noble gases.
C) nucleons.
D) ions.

Question 21

An anion is

A) an element that has lost protons.
B) an element that has gained protons.
C) an element that has lost electrons.
D) an element that have gained electrons.

Question 22

An element with 7 electrons in its outer shell is in which group on the periodic table?

A) Group 5A
B) Group 7A
C) Group 6A
D) Group 2A

Question 23

An electron-dot structure is a convenient method of representing

A) valence electrons of an atom.
B) core electrons of an atom.
C) all electrons of the atom.
D) the complete electron configuration of the atom.

Question 24

When a freshly cut piece of sodium metal, Na, is dropped into a flask with chlorine gas, a violent reaction takes place creating a new compound. This compound

A) has properties that are more like Na than Cl.
B) has properties that are totally unlike either Na or Cl.
C) has properties that more like Cl than Na.
D) has properties that are like both Cl and Na.

Question 25

Which is the electron dot structure of magnesium?

A) Mg
B)
C)
D)

Question 26

Which is the electron dot structure of nitrogen?

A)
B)
C)
D)

Question 27

In a Lewis formula, the dots represent

A) all the electrons in the atoms.
B) the valence electrons in all the atoms.
C) only the electrons that are being transferred or shared.
D) whatever number of electrons are needed to satisfy the octet rule.

Question 28

Which is the electron dot structure of oxygen?

A)
B)
C)
D)

Question 29

The attraction between positive and negative ions is known as a(n)

A) covalent bond.
B) crystal bond.
C) ionic bond.
D) molecular bond.

Question 30

Why do chemists use the Lewis symbols to represent chlorine and sodium rather than drawing the electron diagrams of each element before and after the reaction?

A) Lewis symbols are easier to use.
B) Lewis symbols are more scientific.
C) Lewis symbols are more accurate.
D) Lewis symbols are more abstract.

Question 31

When ions arrange themselves in an orderly structure, that structure is known as a

A) crystal.
B) dipole.
C) molecule.
D) tetrahedron.

Question 32

Where does an element X with the electron dot structure fit in the periodic table?

A) Group 1A
B) Group 2A
C) Group 3A
D) Group 5A

Question 33

From the periodic table, the number of valence electrons for most of the main group elements may be determined directly from the

A) atomic number.
B) group number.
C) period number.
D) nucleon number.

Question 34

How many dots will appear in the Lewis dot structure for an element from in Group 1A of the periodic table?

A) five
B) eight
C) one
D) four

Question 35

Which is the electron dot structure of calcium?

A) Ca
B)
C)
D)

Question 36

With respect to chemical bonding, which particles play the least active role?

A) nucleons
B) core electrons
C) valence electrons
D) All play equal roles.

Question 37

Which of the noble gases does NOT have an octet of electrons in its outer shell?

A) He
B) Ne
C) Ar
D) Kr

Question 38

With respect to chemical bonding, which particles play the most active role?

A) protons
B) neutrons
C) valence electrons
D) core electrons

Question 39

When magnesium combines with bromine, the bond formed is best classified as

A) ionic.
B) polar covalent
C) metallic.
D) nonpolar covalent.

Question 40

Which is the electron dot structure of sulfur?

A)
B)
C)
D) 2

Question 41

When calcium reacts with chlorine, the reaction involves a

A) transfer of electrons from Ca to Cl.
B) transfer of electrons from Cl to Ca.
C) sharing of electrons between Ca and Cl.
D) creation of electrons.

Question 42

Which pair of atoms would form an ionic bond?

A) Na and Mg
B) Ca and S
C) Cl and Br
D) N and N

Question 43

A nitride ion is

A) N⁺.
B) N³⁺.
C) N^2-.
D) N^3-.

Question 44

In reactions to form ionic compounds, metals generally

A) lose electrons.
B) gain electrons.
C) become non-metals.
D) do not react.

Question 45

An oxide ion is

A) O⁺.
B) O²⁺.
C) O^-.
D) O^2-.

Question 46

Calcium reacts with chloride to form

A) CaCl.
B) CaCl₂.
C) Ca₂Cl.
D) Ca₂Cl₃.

Question 47

A sodium ion is

A) Na⁺.
B) Na²⁺.
C) Na^-.
D) Na^2-.

Question 48

A iodide ion is

A) I⁺.
B) I²⁺.
C) I^-.
D) I^2-.

Question 49

Which substance has ionic bonds?

A) O₂
B) BaO
C) H₂O
D) OF₂

Question 50

Chlorine forms monatomic ions with a charge of

A) 1-.
B) 1+.
C) 2-.
D) 2+.

Question 51

In reactions to form ionic compounds, nonmetals generally

A) lose electrons.
B) gain electrons.
C) become metals.
D) do not react.

Question 52

Potassium reacts with iodine to form

A) KI.
B) K₂I.
C) KI₂.
D) K₂I₃.

Question 53

Which atom is least likely to form an ion?

A) bromine, Br
B) phosphorus, P
C) aluminum, Al
D) carbon, C

Question 54

Oxygen forms monatomic ions with a charge of

A) 2+.
B) 3+.
C) 1-.
D) 2-.

Question 55

Which atom is least likely to form an ion?

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

Question 56

When magnesium reacts with chlorine, the reaction involves a

A) transfer of electrons from Mg to Cl.
B) transfer of electrons from Cl to Mg.
C) sharing of electrons between Mg and Cl.
D) creation of electrons.

Question 57

Which substance has ionic bonds?

A) K₂S
B) SO₃
C) CI₄
D) N₂

Question 58

Magnesium reacts with oxygen to form

A) MgO.
B) Mg₂O.
C) MgO₂.
D) Mg₃O₂.

Question 59

Which substance has ionic bonds?

A) Br₂
B) NH₃
C) H₂O
D) LiI

Question 60

When magnesium combines with oxygen, the reaction involves a

A) transfer of electrons from Mg to O.
B) transfer of electrons from O to Mg.
C) sharing of electrons between Mg and O.
D) conversion of protons into electrons.

Question 61

The cation formed when a sodium atom loses an electron is called the

A) sodide ion.
B) sodate ion.
C) sodium ion.
D) soda ion.

Question 62

The formula of aluminum oxide is

A) AlO.
B) AlO₂.
C) AlO₃.
D) Al₂O₃.

Question 63

The anion formed when nitrogen gains three electrons is called the

A) nitride ion.
B) nitrite ion.
C) nitrogide ion.
D) nitro ion.

Question 64

Which is the electron dot structure for nitrogen, N₂?

A)
B)
C)
D)

Question 65

The anion formed when oxygen gains two electrons is called the

A) oxygen ion.
B) oxyide ion.
C) oxide ion.
D) oxy ion.

Question 66

Covalent bonds generally form between

A) ions.
B) metals.
C) metals and nonmetals.
D) nonmetals.

Question 67

Which of the following is a binary compound?

A) HCN
B) O₂
C) LiBr
D) Na₂SO₄

Question 68

The name of the compound with the formula AlCl₃ is

A) aluminum(III) chloride.
B) aluminum trichloride.
C) monoaluminum trichlorine.
D) aluminum chloride.

Question 69

The prefix which means seven is

A) hexa.
B) hepta.
C) octa.
D) tetra.

Question 70

The formula of magnesium nitride is

A) Mg₃N₂.
B) Mg₂N₃.
C) Mg₂N.
D) MgN.

Question 71

An ionic bond is formed when electrons are

A) transferred.
B) shared.
C) split.
D) destroyed.

Question 72

In a molecule of nitrogen, N₂, the nitrogen atoms are bonded to each other by

A) an ionic bond.
B) a single covalent bond.
C) a double covalent bond.
D) a triple covalent bond.

Question 73

The formula for the compound calcium bromide is

A) CaBr.
B) Ca₂Br.
C) CaBr₂.
D) Ca₃Br₂.

Question 74

For which atom is it difficult to predict the most probable ionic charge using the periodic table?

A) H
B) Fe
C) O
D) Ne

Question 75

A covalent bond is formed when a pair of electrons is

A) transferred.
B) shared.
C) split.
D) destroyed.

Question 76

How many electrons are there in a double bond?

A) 1
B) 2
C) 4
D) 6

Question 77

If two atoms from the same element share three pairs of electrons in forming a molecule the bond is called a

A) single covalent bond.
B) double covalent bond.
C) triple covalent bond.
D) coordinate covalent bond.

Question 78

The name of the compound S₂O₃ is

A) disulfur oxide.
B) disulfur trioxide.
C) sulfur oxide.
D) sulfur trioxide.

Question 79

For which atom is it difficult to predict the most probable ionic charge using the periodic table?

A) Co
B) K
C) Al
D) Br

Question 80

Octet means

A) stable electrons.
B) valence electrons.
C) eight.
D) filled shell.