Deck 4: Bonding and Reactions

Question 1

What symptoms did Peggy Carr complain of that made doctors think she might have been poisoned?

A)Numbness in her feet and hands
B)A burning sensation in her extremities
C)Dizziness and nausea
D)Vomiting and profuse sweating

Answer 1

B

Question 2

What ionic compound was found in George Trepal's garage?

A)Thallium(I) triflate
B)Thorium(I) nitrate
C)Thallium(I) nitrate
D)Thallium(I) sulfate

Answer 2

C

Question 3

What have thallium compounds been used for, historically?

A)Rat poison
B)Fertilizer
C)Drain cleaner
D)Drug supplements

Answer 3

A

Question 4

What is the name of the column in the periodic table that includes H, Li, and K?

A)The main group metals
B)The transition metals
C)The alkaline earth metals
D)The alkali metals

Question 5

U and Th are atomic symbols for elements that fall into what group on the periodic table?

A)Transition metals
B)Outer transition metals
C)Inner transition metals
D)Main group metals

Question 6

The alkaline earth metals include which of the following?

A)Mg, Ca, and Sr
B)Mg, Cu, and Sr
C)Mn, Ca, and Sr
D)Mn, Cu, and Sn

Question 7

Silver and gold are examples of what type of element?

A)Main group non-metals
B)Representative metals
C)Main group metals
D)Transition metals

Question 8

Ne, Ar, and Xe are what type of elements?

A)Main group non-metals
B)Noble gases
C)Main group metalloids
D)Noble metals

Question 9

Cl, Br, and I are examples of what type of elements?

A)Halogens
B)Main group gases
C)Noble gases
D)Pnicogens

Question 10

O, N, and F are all what type of element?

A)Transition non-metal
B)Main group metal
C)Transition metal
D)Main group non-metal

Question 11

What do Sc, Mn, and Os have in common?

A)They are all main group metal elements.
B)They are all representative elements.
C)They are all transition metal elements.
D)They are all alkaline earth elements.

Question 12

When a compound forms because an electron or electrons is transferred from one element to another, it is referred to as what type of compound?

A)Ionic
B)Covalent
C)Metallic
D)Coordinate covalent

Question 13

What is the best way to describe all of the following: Mg, Ca, Be?

A)They are compounds.
B)They are elements.
C)They are gaseous elements.
D)They are alkaline earth elements.

Question 14

Which of the following are transition metals?

A)Mg, Ca, Sr
B)Fe, Mn, Ni
C)Pd, Pb, P
D)Sn, Sb, S

Question 15

When electrons are shared between two atoms' outer electron shells, what kind of bond forms?

A)An ionic bond
B)A covalent bond
C)A metallic bond
D)A coordinate covalent bond

Question 16

What is the formula for the compound carbon tetrabromide?

A)CBr
B)CBr₄
C)CBr₃
D)CBr₂

Question 17

The covalent compound sulfur trioxide has what formula?

A)SO₂
B)SO₃
C)SO
D)SO₄

Question 18

What is the formula of the compound dihydrogen selenide?

A)H₂Se
B)HSe₂
C)H₂S
D)HS₂

Question 19

What is the name of SF₄?

A)Sulfur difluoride
B)Tetrasulfur fluoride
C)Tetrafluoro sulfide
D)Sulfur tetrafluoride

Question 20

The compound BrCl goes by what name?

A)Monochloro monobromide
B)Chloro monobromide
C)Bromo monochloride
D)Chloro bromide

Question 21

Where do the shared electrons in a covalent bond tend to be found?

A)Closer to the less electronegative element
B)Closer to the more electronegative element
C)Equally spaced between both elements in the bond
D)At the more electronegative element in the bond

Question 22

Lye is the common name for what chemical?

A)H₂O
B)NaOH
C)HCl
D)C₂H₅OH

Question 23

Oxygen usually refers to what formula for the element?

A)O₃
B)O₄
C)O
D)O₂

Question 24

How does the formation of a covalent bond occur?

A)By the overlap of two atoms electron orbitals
B)By the loss and gain of at least one electron from two atoms
C)By the loss and gain of no more than one electron from each of two atoms
D)By the creation of a new atomic orbital between two atoms

Question 25

What must each name of a covalent compound contain?

A)Enough information to determine the different elements in the compound
B)Two different elements, possibly in a whole number ratio
C)Sufficient numbering to determine the number of atoms in the compound
D)Sufficient information to determine an exact compound

Question 26

In the compound dichlorodifluoromethane, how many chlorine atoms does the name indicate are present?

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

Question 27

The name of this ion, Sr²⁺, is strontonium.

Question 28

What is the name of this chemical species O^2-?

A)Oxonium ion
B)Oxide ion
C)Oxygen ion
D)Oxide atom

Question 29

What is the name of He⁺?

A)Helioid ion
B)Helium ion
C)Helium atom
D)It has no name because it doesn't exist.

Question 30

What is the proper name for Br^- ?

A)The bromide ion
B)The bromine ion
C)The bromonium ion
D)The bromic ion

Question 31

An ionic compound made from calcium and oxygen has what formula?

A)Ca₂O
B)CaO₂
C)Oca
D)CaO

Question 32

What formula does an ionic compound made from aluminum and chlorine have?

A)AlCl₂
B)AlCl₃
C)Al₂Cl
D)Al₃Cl

Question 33

What is the correct formula of an ionic compound made from phosphorus and calcium?

A)CaP₂
B)Ca₂P
C)Ca₃P₂
D)Ca₂P₃

Question 34

What is the correct ionic formula of a compound made from Fe²⁺ and oxygen?

A)Fe₂O₂
B)FeO₂
C)Fe₂O
D)FeO

Question 35

A compound made from Ag⁺ and chlorine has what formula?

A)Ag₂Cl
B)AgCl₂
C)AgCl₃
D)AgCl

Question 36

What formula does an ionic compound made from Cu²⁺ and nitrogen possess?

A)CuN
B)Cu₃N₂
C)Cu₂N₃
D)Cu₃N₃

Question 37

What is the name of the ion, CN^-?

A)The cyanide ion
B)The cyanate ion
C)The sulfate ion
D)The sulfite ion

Question 38

What is the formula for an ionic compound made from magnesium and nitrate?

A)Mg(NO₃)₂
B)MgNO₃
C)Mg₂NO₃
D)(Mg)₂NO₃

Question 39

Ionic compounds all have what two physical properties?

A)Plasticity and rigidity
B)Hardness and amorphousness
C)Plasticity and amorphousness
D)Hardness and rigidity

Question 40

What must be included in the formula of any ionic compound?

A)Three or more elements
B)Positive and negative ionic charges
C)A cation and an anion, written cation first, followed by anion
D)Two or more elements, as well as positive and negative ionic charges

Question 41

In the salt KCN, what is the anion?

A)K⁺
B)C²⁺
C)CN^-
D)N^3-

Question 42

What do all cations have in common?

A)Positive charge.
B)They are formed from a single atom.
C)They are metallic elements.
D)None of the above.

Question 43

Which of the following are ionic compounds?

A)CH₄ and CCl₄
B)NH₃ and PH₃
C)H₂O and H₂S
D)None of the above. They are all examples of covalent compounds.

Question 44

Diatomic elements have how many elements and how many atoms in their formula?

A)One element and one atom
B)One element and two atoms
C)Two elements and one atom
D)Two elements and two atoms

Question 45

Dihydrogen monoxide is the best systematic name for what common substance?

A)Water
B)Ammonia
C)Salt
D)Alcohol

Question 46

What is the common name for dihydrogen monoxide?

A)Swamp gas
B)Water
C)Alcohol
D)Ethanol

Question 47

HCl has what common name?

A)Muriatic acid
B)Table salt
C)Oil of vitriol
D)Alcohol

Question 48

What physical sense is not used in helping determine what an unknown substance might be?

A)Sight
B)Touch
C)Smell
D)Taste

Question 49

The products of a chemical reaction are commonly listed where?

A)In the middle of a chemical reaction
B)On the left of a chemical reaction
C)On the right of a chemical reaction
D)At either end of a chemical reaction

Question 50

Why can't a chemical equation be balanced by changing the subscripts of the reactants and/or products?

A)Because there will always be more reactants than products when using such a method.
B)Because changing the subscripts means changing the identity of the chemicals.
C)It just can't!
D)None of the above; it can be balanced in this manner.

Question 51

When the reactants and products of a chemical equation are known, how is it then balanced?

A)By adjusting and changing the coefficients of the equation
B)By adjusting and changing the subscripts of the equation
C)By doubling either the reactants or the products
D)By adjusting or changing both the coefficients and he subscripts of the equation

Question 52

What is the balanced form of this equation: H₂ + Cl₂ → HCl?

A)H₂ + Cl₂ → 2 HCl
B)H₂ + Cl₂ → H₂Cl₂
C)2 H + 2 Cl → 2 HCl
D)2 H + 2 Cl → H₂Cl₂

Question 53

How does the equation Fe + O₂ → Fe₂O₃ appear when properly balanced?

A)4 Fe + 6 O → Fe₄O₆
B)Fe + O₂ → Fe₂O₃
C)4 Fe + 3 O₂ → 2 Fe₂O₃
D)2 Fe + 3 O₂ → 2 Fe₂O₃

Question 54

How does the following appear when properly balanced: CH₄+ O₂ → CO₂ + H₂O?

A)2 CH₄ + O₂ → 2 CO₂ + H₂O
B)CH₄ + 2 O₂ → CO₂ + H₂O
C)CH₄ + 2 O₂ → CO₂ + 2 H₂O
D)CH₄ + O₂ → CO₂ + 2 H₂O

Question 55

How is this equation balanced: Si + O₂ → SiO₄?

A)2 Si + O₂ → SiO₄
B)Si + O₄ → SiO₄
C)Si + O₂ → 2 SiO₄
D)Si + 2 O₂ → SiO₄

Question 56

How does this appear when properly balanced: NaClO₃ → O₂ + NaCl?

A)2 NaClO₃ → O₂ + 2 NaCl
B)2 NaClO₃ → 3 O₂ + 2 NaCl
C)2 NaClO₃ → 3 O₂ + NaCl
D)NaClO₃ → 3 O₂ + 2 NaCl

Question 57

What does Avogadro's number, 6.20 × 10²³, indicate?

A)The known quantity of atoms in a mass of a compound
B)The known quantity of atoms in a mass of an element
C)The known quantity of atoms in the atomic mass of an element
D)Nothing, really, just the number of atoms he counted in a sample of an element

Question 58

What is the mass of 0.5 mole of S atoms?

A)16 g
B)32 g
C)8.0 g
D)0.5 g

Question 59

What is the mass of 2.0 moles of silver?

A)2.0 g
B)216 g
C)108 g
D)54 g

Question 60

The mass of 3.0 moles of NaCl is what?

A)3.00 g
B)175.5 g
C)58.5 g
D)19.0 g

Question 61

What is the mass of 5.0 moles of CH₄?

A)80 g
B)3.2 g
C)21.0 g
D)16 g

Question 62

How many moles are in 64 g of CH₄?

A)2.0 moles
B)4.0 moles
C)16 moles
D)76 moles

Question 63

How many moles are in 12.0 g of helium?

A)48.0 moles
B)16.0moles
C)3.0 moles
D)8.0 moles

Question 64

How many moles of material are in 74.5 g of KCl?

A)1.0 mole
B)2.0 moles
C)0.5 moles
D)74.5 moles

Question 65

How many moles of water does 72.0 g of it contain?

A)72.0 moles
B)2.0 moles
C)4.0 moles
D)1.0 moles

Question 66

116 g of isopropanol, formula C₃H₈O, contains how many moles?

A)58.0 moles
B)1.0 moles
C)1.5 moles
D)2.0 moles

Question 67

In the reaction: 2 Na + Cl₂ → 2 NaCl, if 46.0 g of sodium react, what is the first step necessary in determining how much sodium chloride can form?

A)Computing the number of atoms of sodium
B)Computing the number of moles of chlorine
C)Computing the number of grams of chlorine
D)Computing the number of moles of sodium

Question 68

How is stoichiometry best defined?

A)The use of chemical equations for determining the materials in a given chemical calculation
B)The use of balanced chemical equations for identifying the materials in a given chemical reaction
C)The use of unbalanced chemical equations for quantifying the amount of materials in a given chemical reaction
D)The use of balanced chemical equations for quantifying the amount of materials in a given chemical reaction

Question 69

How many grams of HCl are produced according to the following equation, H₂ + Cl₂ → 2 HCl, when 4.0 g of hydrogen reacts completely?

A)72.0 g
B)144 g
C)2.0 g
D)36.0 g

Question 70

How many grams of water are produced if 32.0 g of CH₄ are completely consumed, according to the equation CH₄ + 2 O₂ → CO₂ + 2 H₂O?

A)0.22 g
B)32.0 g
C)72.0 g
D)36.0 g

Question 71

If 78.0 g of potassium are consumed to make KCl according to the equation 2 K + Cl₂ → 2 KCl, how much product can form?

A)149 g
B)0.023 g
C)40.8 g
D)78.0 g

Question 72

How many grams of O₂ are needed to react completely with 28.0 g of Li in the following, 2 Li + O₂ → Li₂O?

A)64.0 g
B)32.0 g
C)7.0 g
D)256.0 g

Question 73

When O₂ reacts with C₂H₆, according to the equation 2 C₂H₆ + 7 O₂ → 4 CO₂ + 6 H₂O, how much CO₂ is produced from 60.0 g of C₂H₆?

A)60.0 g
B)44.0 g
C)88.0 g
D)176 g

Question 74

If HI reacts completely in the reaction KOH + HI → H₂O + KI, how much KOH is needed to react with 128 g of HI?

A)112 g
B)56.0 g
C)128 g
D)256 g

Question 75

How much NaBr is needed to react completely with 100.0 g of AgNO₃, according to the equation NaBr + AgNO₃ → AgBr + NaNO₃?

A)30.7 g
B)122.6 g
C)61.3 g
D)100.0 g

Question 76

In the reaction 2 Na + Cl₂ → 2 NaCl, how much sodium chloride can be produced from 235.0 g of Cl₂?

A)235.0 g
B)193.3 g
C)387.3 g
D)96.8 g

Question 77

When calcium carbonate decomposes, according to the equation CaCO₃ → CaO + CO₂, how many grams of CO₂ are produced from the decomposition of 520.0 g of CaCO₃?

A)228.8 g
B)457.6 g
C)520.0 g
D)114.4 g

Question 78

What do the combustion of gasoline and the rusting of iron have in common?

A)Both occur on a long time scale.
B)Both are single replacement reactions.
C)Both are metathesis reactions.
D)Both are redox reactions.

Question 79

What are the common products of neutralization reactions?

A)Acids and bases
B)Ionic compounds
C)Water and a salt
D)Gases and liquids

Question 80

What type of reaction is the following: 2 Na + Cl₂ → 2 NaCl?

A)An oxidation-reduction reaction
B)A decomposition reaction
C)A combustion
D)A precipitation reaction