Chem Test (11/27)

True or False Boron trifluoride has three bonding domains, and its electron domain geometry is trigonal planar.

True

True or False Electron affinity is a measure of how strongly an atom can attract additional electrons.

True

True or False Electron affinity measures how easily an atom gains an electron.

True

True or False Elements that readily conduct electricity are elements with low ionization energies.

True

True or False Hybridization is the process of mixing atomic orbitals as atoms approach each other to form a bond.

True

True or False In some molecules and polyatomic ions, the sum of the valence electrons is odd and as a result the octet rule fails.

True

True or False Most transition metals do not form ions with a noble gas configuration.

True

True or False The greater the lattice energy, the greater the charges on the participatory ions and the smaller their radii.

True

A ________ covalent bond between the same two atoms is the longest. a. single b. double c. triple d. They are all the same length.

a

Ca reacts with element X to form an ionic compound with the formula CaX. Al will react with X to form ________. a. Al2X3 b. Al3X2 c. AlX2 d. AlX

a

Of the bonds below, ________ is the most polar. a. Na-Cl b. Na-S c. P-S d. Si-Cl

a

The electron domain and molecular geometry of NF3 are ________. a. tetrahedral, trigonal pyramidal b. tetrahedral, tetrahedral c. octahedral, octahedral d. octahedral, square pyramidal

a

The first ionization energies of the elements ________ as you go from left to right across a period of the periodic table, and ________ as you go from the bottom to the top of a group in the table. a. increase, increase b. increase, decrease c. decrease, increase d. decrease, decrease

a

The only noble gas that does not have the ns2np6 valence electron configuration is ________. a. helium b. neon c. radon d. All noble gases have the ns2np6 valence electron configuration.

a

The type of compound that is most likely to contain a covalent bond is ________. a. one that is composed of only nonmetals b. held together by the electrostatic forces between oppositely charged ions c. one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table d. There is no general rule to predict covalency in bonds.

a

What is the maximum number of double bonds that a hydrogen atom can form? a. 0 b. 1 c. 2 d. 3

a

________ have the lowest first ionization energies of the groups listed. a. Alkali metals b. Noble gases c. Halogens d. Alkaline earth metals

a

A tin atom has 50 electrons. Electrons in the ________ subshell experience the lowest effective nuclear charge. a. 5s b. 5p c. 3d d. 3p

b

According to valence bond theory, which orbitals overlap in the formation of the bond in HI a. 1s on H and 5s on I b. 1s on H and 5p on I c. 2s on H and 5p on I d. 1s on H and 6p on I

b

An antibonding π orbital contains a maximum of ________ electrons. a. 1 b. 2 c. 4 d. 6

b

In the Lewis structure of ClF, the formal charge on Cl is ________, and the formal charge on F is ________. a. -1, -1 b. 0, 0 c. -1, +1 d. +1, -1

b

In the Lewis symbol for a nitrogen atom, there are ________ paired and ________ unpaired electrons. a. one, three b. two, three c. zero, five d. three, two

b

Ni2+ ions are represented by the electron configuration ________. a. [Ar]4s23d6 b. [Ar]3d8 c. [Ar]3d6 d. [Ar]3d10

b

Of the following, only ________ has sp2 hybridization of the central atom. a. CO2 b. SO3 c. ICl3 d. NF3

b

Of the molecules below, only ________ is polar. a. F2 b. AsH3 c. SF6 d. CF4

b

The H-C-H bond angle in the CH4 molecule is approximately ________. a. 90 b. 109.5 c. 180 d. 60

b

The ________ have the most negative electron affinities. a. transition metals b. halogens c. alkaline earth metals d. alkali metals

b

The combination of two atomic orbitals results in the formation of ________ molecular orbitals. a. 1 b. 2 c. 3 d. 4

b

The hybrid orbital set used by the central atom in SO2 is ________. a. sp b. sp2 c. sp3 d. sp3d

b

The oxidation number of phosphorus in PF3 is ________. a. +2 b. +3 c. 0 d. -3

b

There are ________ σ and ________ π bonds in the H - C≡C - H molecule. a. 5 and 0 b. 3 and 2 c. 2 and 3 d. 4 and 3

b

What is the coefficient of H2O when the following equation is completed and balanced? Ba (s) + H2O (l) → a. 1 b. 2 c. 3 d. Ba (s) does not react with H2O (l).

b

What is the maximum number of triple bonds that a carbon atom can form? a. 0 b. 1 c. 2 d. 3

b

Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br a. O, Se b. Sr c. Na d. Br

b

Which one of the following atoms has the largest radius? a. C b. B c. N d. F

b

Electronegativity ________ from left to right within a period and ________ from top to bottom within a group. a. increases, stays the same b. decreases, increases c. increases, decreases d.stays the same, increases

c

Resonance structures differ by ________. a. number and placement of electrons b. number of atoms only c. placement of electrons only d. number of electrons only

c

The central atom in the SnCl3- ion has ________ nonbonded electron pair(s) and ________ bonded electron pair(s) in its valence shell. a. 6, 2 b. 3, 2 c. 1, 3 d. 0, 4

c

The hybrid orbital set used by the central atom in BrO3- is ________. a. sp b. sp2 c. sp3 d. sp3d

c

The most electronegative atom of the ones listed below is ________. a. S b. P c. Cl d. Si

c

There are ________ valence electrons in the Lewis structure of CH3OH. a. 18 b. 22 c. 14 d. 20

c

There are ________ σ and ________ π bond(s) in the H2C=CH2 molecule. a. 3 and 4 b. 3 and 2 c. 5 and 1 d. 4 and 3

c

What is the maximum number of double bonds that a carbon atom can form? a. 0 b. 1 c. 2 d. 4

c

Which two bonds are least similar in polarity? a. B-F and Cl-F b. C-Cl and Ge-Cl c. Al-Cl and I-Br d. I-Br and Si-Cl

c

According to MO theory, overlap of two p atomic orbitals produces ________. a. one π MO and one σ MO b. two π MOs, two π+ MOs, one σ MO, and one σ* MO c. one π+ MO and one σ* MO d. one π MO and one π* MO or one σ MO and one σ* MO

d

According to VSEPR theory, if there are six electron domains in the valence shell of an atom, they will be arranged in a(n) ________ geometry. a. tetrahedral b. trigonal planar c. trigonal bipyramidal d. octahedral

d

According to valence bond theory, which orbitals overlap in the formation of the bond in Br2? a. 3s b. 3p c. 4s d. 4p

d

According to valence bond theory, which orbitals overlap in the formation of the bond in BrI a. 5p on Br and 6p on I b. 3p on Br and 4p on I c. 5s on Br and 7s on I d. 4p on Br and 5p on I

d

As the number of covalent bonds between two atoms increases, the distance between the atoms ________ and the strength of the bond between them ________. a. increases, increases b. decreases, decreases c. increases, decreases d. decreases, increases

d

Atomic radius generally increases as we move ________. a. down a group and from left to right across a period b. down a group; the period position has no effect c. up a group and from right to left across a period d.down a group and from right to left across a period

d

How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? a. 1 b. 2 c. 3 d. 4

d

How many single covalent bonds must a carbon atom form to have a complete octet in its valence shell? a. 0 b. 1 c. 3 d. 4

d

In nature, the noble gases exist as ________. a. the sulfides b. the gaseous fluorides c. solids in rocks and in minerals d. monatomic gaseous atoms

d

In which of the following atoms is the 2s orbital closest to the nucleus? a. C b. N c. O d. F

d

The ________ ion has a noble gas electron configuration. a. Be+ b. B4+ c. Al3- d. B3+

d

The basis of the VSEPR model of molecular bonding is ________. a. regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap b. atomic orbitals of the bonding atoms must overlap for a bond to form c. regions of electron density on an atom will organize themselves so as to maximize s-character d. electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions

d

The central atom in ________ violates the octet rule. a. ClCN b. OBr2 c. N2 d. BF3

d

The list that correctly indicates the order of metallic character is ________. a. F > Cl > S b. P > S > Se c. Na > K > Rb d. Si > P > S

d

There are ________ paired and ________ unpaired electrons in the Lewis symbol for a sulfur atom. a. 4, 1 b. 0, 5 c. 2, 5 d. 4, 2

d

True or False Electron domains for single bonds exert greater force on adjacent domains than the electron domains for multiple bonds.

False

True or False Electrons in core orbitals contribute to atom bonding.

False

True or False Possible shapes of AB3 molecules are linear, trigonal planar, and T-shaped.

False

True or False XeF4 is a polar molecule.

False