Honors Chem Chp 8 Test Review

tetrahedral angle

109.5 degrees

What is the ending for the names of all binary compounds, both ionic and molecular? a. -ide b. -ade c. -ate d. -ite

A (-ide)

How many valid electron dot formulas--having the same number of electron pair for a molecule or ion--can be written wihen a resonance structure occurs? a. 0 b. 2 only c. 1 only d. 2 or more

A (0)

What is the formula unit for aluminum oxide? a. Al2O3 b. AlO c. Al3O d. AlO3

A (Al2O3)

What is the formula for sulfurous acid? a. H2SO3 b. H2SO4 c. H2SO2 d. H2S

A (H2SO3)

7. Which of the following pairs of substances best illustrates the law of multiple proportions? a. NO and NO2 b. CaCl2 and CaBr2 c. H2 and O2 d. P2O5 and PH3

A (NO and NO2)

Which of these elements does not exist as a diatomic molecule? a. Ne b. I c. H d. F

A (Ne)

3. Which of the following is a binary molecular compound? a. P Cl5 b. Be H C O3 c. Mn O d. Mn Br2

A (P Cl5)

An -ate or -ite at the end fo a compound name usually indicates that the compound contains________. a. a polyatomic anion b. fewer electrons than protons c. netural molecules d. only two elements

A (a polyatomic anion)

What is required in order to melt a network solid? a. breaking covalent bonds b. breaking Van der Waals bonds c. breaking hydrogen bonds d. braking ionic bonds

A (breaking covalent bonds)

Which of the following correctly provides the name of the element, the symbol for the ion, and the name of the ion? a. copper, Cu+, cuprous ion b. sulfur, S2-, sulfurous ion c. flourine, F+, fluoride ion d. zinc, Zn2+, zincate ion

A (copper, Cu+, cuprous ion)

Which of the forces of molecular attraction is the weakest? a. dispersion b. dipole interaction c. single covalent bond d. hydrogen bond

A (dispersion)

4. Which of the following particles are free to drift in metals? a. electrons b. neutrons c. protons d. cations

A (electrons)

5. Which of the following elements does NOT form an ion with a charge of 1+? a. fluorine b. potassium c. sodium d. hyrdrogen

A (fluorine)

Why is hydrogen bonding only possible with hyrdrogen? a. hydrogen's nucleus is electron deficient when it bonds with an electronegative atom b. hydrogen is the only atom that is the same size as an oxygen atom c. hydrogen is the most elecrotnegative element d. hydrogen tends to form covalent bonds

A (hyrdrogen's nucleus is electron deficient when it bonds with an electronegative atom)

Which set of chemical name and chemical formula for the same compound is correct? a. iron (III) phospate, FePO4 b. lithium carbonate, LiCO3 c. ammonium sultite, (NH4)2S d. magnesium dichromate, MgCrO4

A (iron (III) phospate, FePO4)

Suppose you encounter a chemical formula with H as the cation. What do you know about this compound immediately? a. it is an acid. b. it is a polyatomic ionic compound c. it is a base d. it has a +1 charge

A (it is an acid)

What determines that an element is a metal? a. its position in the periodic table b. the magnitude of its charge c. the molecules that it forms d. when it is a Group A element

A (its position in the periodic table)

Which noble gas has the same electron configuration as the oxygen in a water molecule? a. neon b. argon c. xenon d. helium

A (neon)

Which polyatoimc ion forms a neutral compound when combined with a group 1A monatoimc ion in a 1:1 ratio? a. nitrate b. carbonate c. phosphate d. hydroxide

A (nitrate)

Which of the following elements can form diatomic molecules held together by triple covalent bonds? a. nitrogen b. carbon c. fluorine d. oxygen

A (nitrogen)

Which of the following correctly shows a prefix used in naming binary molecular compounds with its correspoding number? a. nona,-9 b. deca,-7 c. octa,-4 d. hexa,-8

A (nona,-9)

What causes water moleucle to have a bent shape, according to VSEPR theory? a. repulsive forces between unshared pairs of electrons b. ionic attraction and repulsion c. the unusual location of the free electrons d. interaction between the fixed orbitals of the unshared pairs of oxygen

A (repulsive forces between unshared pairs of electrons)

In which of the following is the name and formula given correctly? a. stannic fluoride, SnF4 b. cobaltous chloride, CoCl3 c. barium nitride, BaN d. sodium oxide, NaO

A (stannic fluoride, SnF4)

What is the name of H2SO3? a. sulfurous acid b. hyposulfuric acid c. sulfuric acid d. hydrosulfuric acid

A (sulfurous acid)

Which of the following is NOT a characteristic of most ionic compounds? a. They have low melting points. b. They are solids. c. When melted, they conduct an electric current. d. They are composed of metallic and nonmetallic elements.

A (they have low melting points)

What is the correct name for Sn3 (PO4)2? a. tin (II) phosphate b. tin (III) phosphate c. tritin diphospate d. tin (IV) phosphate

A (tin (II) phosphate)

Why do atoms share electrons in covalent bonds? a. to attain a noble-gas electron configuration b. to become ions and attract each other c. to increase their atomic numbers d. to become more polar

A (to attain a noble-gas electron configuration)

How many valence electrons are transferred from the nitrogen atom to potassium in the formation of the compound potassium nitride? a. 1 b. 0 c. 2 d. 3

B (0)

What is the electron configuration of the oxide ion (O2-)? a. 1s2 2s2 b. 1s2 2s2 2p6 c. 1s2 2s2 2p2 d. 1s2 2s2 2p4

B (1s2 2s2 2p6)

Alloys are commonly used in manufacturing. Which of the following is NOT a reason to use an alloy instead of a pure metal? a. Brass is more malleable than pure copper b. Cast iron is more brittle than pure iron c. Bronze is tougher than pure copper d. Sterling silver is stronger than pure silver

B (Cast iron is more brittle than pure iron)

A molecule with a single covalent bond is____. a. CO2 b. Cl2 c. N2 d. CO

B (Cl2)

2. Which of the following compounds contains the Mn3+ ion? a. MnS b. Mn2 O3 c. MnO d. Mn Br2

B (Mn2 O3)

What is the formula for sodium sulfate? a. Na(SO4)2 b. Na2SO4 c. Na2(SO4)2 d. NaSO4

B (Na2SO4)

8. What is the formula of the ion formed when phosphorus achieves a noble-gas electron configuration? a. P3+ b. P3- c. P2+ d. P2-

B (P3-)

Which of the following compounds contains the lead (II) ion? a. Pb2S b. PbO c. PbCl4 d. Pb2O

B (PbO)

In which of the following are the formula of the ionic compound and the charge on the metal ion shown correctly? a. NiO, Ni+ b. ThO2, Th4+ c. UCl5, U+ d. IrS2, Ir2+

B (ThO2, Th4+)

When H+ forms a bond with H2O to form the hydronium ion of H3O+, this bond is called a coordinate covalent bond because _______. a. it forms an especially strong bond b. both bonding electrons come from the oxygen atom c. the electrons are equally shared d. the oxygen no longer has eight valence electrons

B (both bonding electrons come from the oxygen atom)

How is a pair of molecular orbitals formed? a. by the overlap of two atomic orbitals from the same atom b. by the overlap of two atomic orbitals from different atoms c. by the splitting of a single atomic orbital d. by the reproduction of a single atomic orbital

B (by the overlap of two atomic orbitals from different atoms)

Which of the following is the correct name for N2O5? a. nitrous oxide b. dinitrogen pentaoxide c. nitrogen dioxide d. nitrate oxide

B (dinitrogen pentaoxide)

Which elements can form diatomic molecules joined by a single covalent bond? a. hydrogen only b. hyrdrogen and the halogens only c. halogens only d. halogens and members of the oxygen group only

B (hydrogen and the halogens only)

What is the correct name for the N3- ion? a. nitrogen ion b. nitride ion c. nitrite ion d. nitrate ion

B (nitride ion)

Which of the following occurs in an ionic bond? a. like-charged ions attract b. oppositely charged ions attract c. two atoms share two electrons d. two atoms share more than two electrons

B (oppositely charged ions attract)

Which of the following bond types is normally the weakest? a. sigma bond formed by the overlap of one s and one p orbital b. pi bond formed by the overlap of two p orbitals d. sigma bond formed by the overlap of two s orbitals

B (pi bond formed by the overlap of two p orbitals)

Sigma bonds ar formed as a relsult of the overlapping of which type(s) of atomic orbital(s)? a. p only b. s and p c. s only d. d only

B (s and p)

Ionic compounds are normally in which physical state at room temperature? a. liquid b. solid c. plasma d. gas

B (solid)

Which set of chemical name and chemical formula for the same compound is correct? a. aluminum fluorate, AlF3 b. tin (IV) bromide, SnBr4 c. iron (II) oxide, Fe2O3 d. potassium chloride, K2Cl2

B (tin (IV) bromide, SnBr4)

Which of the following is the name given to the pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules? a. Outer pair b. unshared pair c. unvalenced pair d. inner pair

B (unshared pair)

How many valence electrons are in an atom of magnesium? a. 5 b. 4 c. 2 d. 3

C (2)

How many valence electrons are transferred from the calcium atom to iodine in the formation of the compound calcium iodide? a. 1 b. 0 c. 2 d. 3

C (2)

How many valence electrons are in an atom of phosphorus? a. 4 b. 3 c. 5 d. 2

C (5)

Which of the following correctly represents an ion pair and the ionic compound the ions form? a. Pb4+, O2-; Pb2O4 b. Na+, Cl-; NaCl2 c. Ca2-, F-; CaF2 d. Ba2+, O2-; Ba2O2

C (Ca2-, F-; CaF2)

In which of the following are the symbol and name for the ion given correctly? a. Sn2+: stannic ion; Sn4+: stannous ion b. PBb+: lead ion; Pb4+: lead (IV) ion c. Fe2+: ferrous ion; Fe3+: ferric ion d. Co2+: cobalt (II); Co3+: cobaltous ion

C (Fe2+: ferrous ion; Fe3+: ferric ion)

What is the correct formula for potassium sulfite? a. KHSO4 b. K2SO4 c. K2SO3 d. KHSO3

C (K2SO3)

In which of the following are the symbol and name for the ion given correclty? a. NH4+: ammonia, H+: hydride b. PO3 3-: phospate; PO4 3-: phosphite c. OH-: hydroxide; O2-: oxide d. C2H3O2-: acetate; C2O4-: oxalite

C (OH-: hydroxide; O2-: oxide)

In which of the following compounds is the octet expanded to include 12 electrons? a. PCl3 b. H2S c. SF6 d. PCl5

C (SF6)

Select the correct formula for sulfer hexaflouride. a. F6SO3 b. F6S2 c. SF6 d. S2F6

C (SF6)

What causes dipole interactions? a. sharing of electron pairs b. bonding of a covalently bonded hyrdogen to an unshared electron pair c. attraction between polar molecules d. attraction between ions

C (attraction between polar molecules)

Sulfur hexafluoride is an example of a ______. a. monatomic ion b. polyatomic ion c. binary compound d. polyatomic ion

C (binary compound)

Which metallic crystal structure has a coordination number of 8? a. hexagonal close-packing b. face-centered cubic c. body-centered cubic d. tetragonal

C (body-centered cubic)

The nonmetals in Groups 6A and 7A ______. a. end in -ate b. all have ions of -1 charge c. have a numerical charge that is found by subtracting 8 from the group number d. lose electrons when they form ions

C (have a numerical charge that is found by subtracting 8 from the group number)

How does oxygen obey the octet rule when reacting to form compounds? a. it gives up electrons b. oxygen does not obey the octet rule c. it gains electrons d. it does not change its number of electrons

C (it gains electrons)

6. What is the name of the ionic compound formed from lithium and bromine? a. lithium bromine b. lithium bromate c. lithium bromide d. lithium bromium

C (lithium bromide)

Under what conditions can potassium bromide conduct electricity? a. only when it is in crystal form b. only when melted c. only when melted or dissolved in water d. only when dissolved

C (only when melted or dissolved in water)

Which of the following theories provides information concerning both molecular shape and molecular bonding? a. VSEPR theory b. molecular orbital theory c. orbial hybridization theory d. Bohr atomic theory

C (orbital hybridization theory)

What does an -ite or -ate ending in a polyatomic ion mean? a. sulfur is in the formula b. bromine is in the formula c. oxygen is in the formula d. nitrogen is in the formula

C (oxygen is in the formula)

1. Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen? a. S b. C c. O d. Na

C (oxygen)

what type of compound is CuSO4? a. binary molecular b. monotomic ionic c. polyatomic ionic d. polyatomic covalent

C (poliatomic ionic)

Molecular orbital theory is based upon which of the following models of the atom? a. democritus's model b. bohr model c. quantum mechanical model d. classical mechanical model

C (quantum mechanical model)

What type of hybrid orbital exists in the methane molecule? a. sp b. sp2 c. sp3 d. sp3d2

C (sp3)

Which of the following is true about the composition of ionic compounds? a. They are composed of anions only b. They are composed of cations only c. They are composed of anions and cations d. They are formed from two or more nonmetallic elements

C (they are composed of anions and cations)

Which of the following formulas represents an ionic compound? a. CS2 b. PCl3 c. N2O4 d. BaI2

D (BaI2)

What is the correct name for the compound CoCl2? a. Cobalt (I) chloride b. Cobalt (I) chlorate c. Cobalt (II) chlorate d. Cobalt (II) chloride

D (Cobalt (II) chloride)

Which of the following shows correctly an ion pair and the ionic compound the two ions form? a. Cu2+, O2-; Cu2O2 b. Sn4+, N3-; Sn4N3 c. Cr3+, I-; CrI d. Fe3+, O2-; Fe2O3

D (Fe3+, O2-; Fe2O3)

Which of the following covalent bonds is the most polar? a. H--H b. H--N c. H--C d. H--F

D (H--F)

What is the formula for hydrosulfuirc acid? a. H2SO2 b. H2S2 c. HSO2 d. H2S

D (H2S)

Which of the following is true about an ionic compound? a. It is a salt b. it is held together by ionic bonds c. it is composed of anions and cations d. all of the above

D (all of the above)

What causes hydrogen bonding? a. attraction between ions b. motion of electrons c. sharing of electron pairs d. bonding of a covalently bonded hydrogen atom with an unshared electron pair

D (bonding of a covalently bonded hydrogen atom with an unshared electron pair)

Which of the following correctly provides the names and formulas of polyatomic ions? a. carbonate: HCO3-; biocarbonate: CO32- b. sulfite: S2-; sulfate: SO3- c. nitrite: NO-; nitrate: NO2- d. chromate: CrO42-; dichromate: CrO72-

D (chromate: CrO42-; dichromate: CrO72-)

Why are systematic names preferred over common names? a. common names are derived from the method used to obtain the compound b. common names are not very descriptive c. common names were assigned by the scientists who discovered the compound d. common names do not provide information about the chemical composition of the compound

D (common names do not provide information about the chemical composition of the compound)

Molecular compounds are usually _________. a. composed of a positive and negative ions b. exceptions to the law of definite proportions c. composed of two or more transition elements d. composed of two or more nonmetallic elements

D (composed of two or more nonmetallic elements)

Which of the following are produced when a base is dissoved in water a. hyrdrogen ions b. ammonium ions c. hyrdronium ions d. hyroxide ions

D (hydroxide ions)

Consider a mystery compound having the formula MxTy. If the compound is not an acid, if it contains only two elements, and if M is not a metal, which of the following is true about the compound? a. it contains a polyatomic ion b. its name ends in -ic c. its name ends in -ite or -ate d. it is a binary molecular compound

D (it is a binary molecular compound)

How are bases named? a. like molecular compounds b. like polyatoimc ions c. like monatomic elements d. like ionic compounds

D (like ionic compounds)

What is the shape of a molecule with a triple bond? a. bent b. tetrahedral c. pyramidal d. linear

D (linear)

The side-by-side overlap of p orbital produces what kind of bond? a. sigma bond b. beta bond c. alpha bond d. pi bond

D (pi bond)

Which of the following compounds has the formula KNO3? a. potassium nitride b. potassium nitrite c. potassium nitrogen oxide d. potassium nitrate

D (potassium nitrate)

What type of hybridization occurs in the orbitals of a carbon atom participating in a triple bond with another carbon atom? a. sp2 b. sp3 c. pd d. sp

D (sp)

Which of the following is NOT a cation? a. mercurous ion b. iron(III) ion c. Ca2+ d. sulfate

D (sulfate)

What does the term coordination number in ionic crystals refer to? a. the number of atoms in a particular formula unit b. the number of like-charged ions surrounding a particular ion c. the total number of valence electrons in an atom d. the number of oppositely charge ions surrounding a particular ion

D (the number of oppositely charged ions surrounding a particular ion)

What characteristic of metals makes them good electrical conductors? a. They have mobile protons b. their crystal structures can be rearranged easily c. they have mobile cations d. they have mobile valence electrons

D (they have mobile valence electrons)

polar bond

a covalent bond between two atoms of significantly different eletronegativities

single covalent bond

a covalent bond in which only one pair of electrons is shared

coordinate covalent bond

a covalent bond in which the shared electron pair comes only from one of the atoms

double covalent bond

a covalent bond in which two pairs of electrons are shared

electron dot structure

a depiction of valence electrons around the symbol of an element

hyrdrogen bond

a type of bond that is very important in determining the properties of water and of important biological molecules such as proteins and DNA

halide ion

an anion of chlorine or other halogen

anion

atom or group of atoms having a negative charge

cation

atom or group of atoms having a positive charge

octet rule

atoms react so as to acquire the stable electron structure of a noble gas

dipole interaction

attraction between polar molecules

binary compound

compound composed of two different elements

polyatomic ion

compound composed of two different elements

monatomic ion

consists of a single atoms with a positive or negative charge

bond dissociation energy

energy needed to break a single bond between two covalently bonded atoms

law of definite proportions

in any chemical compound, the masses of elements are always in the same proportion by mass

Bonding orbital

molecular orbital that can be occupied by two electrons of a covalent bond

acid

produces a hydrogen ion when dissolved in water

base

produces a hydroxide ion when dissolved in water

VSEPR theory

shapes adjust so valence-electron pairs are as far apart as possible

sigma bond

symmetrical bond along the axis between the two nuclei

ionic bond

the force of attraction binding oppositely charged ions together

coordination number

the number of ions of opposite charge surrounding each ion in a crystal

law of multiple proportions

when two elements form more than one compound, the masses of one element that combine with the same mass of the other element are in the ratio of small, whole numbers