CHM 113 quiz 3

In the Lewis structure for ICl2-, what is the formal charge on the iodine atom? a) -2 b) -1 c) 0 d) 1

-1

Determine the formal charge on the iodine atom in ICl5. a) +1 b) -1 c) 0 d) 5

0

the values of I for s orbitals is

0

the value of I for p orbitals is

1

How many electrons in an atom can have the quantum numbers n = 3, l = 2? a)2 b)5 c)10 d)18

10

How many unpaired electrons are present in the orbital diagram of Se? a)3 b)1 c)2 d)0

2

the value of I for d orbitals is

2

Select the correct statement for n=5 OrbitalsElectrons a)5 10 b)25 50 c)10 20 d)16 32

25 50

Which of the following is an incorrect designation for an atomic orbital? a)1s b)3d c)2p d)3f

3f

The electron-dot structure of the molecule, SF4, contains a). 1 double bond and 4 single bonds b) 4 single bonds and 13 lone pair electrons. c) 4 single bonds and 12 lone pair electrons. d) 4 single bonds and 1 lone pair electrons

4 single bonds and 13 lone pair electrons

The Lewis structure of the molecule, NH4O+, contains a) 1 double bond and 4 single bonds b) 5 single bonds and 3 lone pair electrons. c) 5 single bonds and 2 lone pair electrons. d) 5 single bonds and 1 lone pair electrons

5 single bonds and 2 lone pair electrons

The orbital diagram for the valence shell of Cl contains _____. a)8 full orbitals and 1 half-filled orbital b)6 paired electrons and 1 unpaired electron c)8 paired electrons d)2 full orbitals and 1 half-filled orbital

6 paired electrons and 1 unpaired electron

h is planck's constant

6.626 x 10^-34 Js

Angstrom

A 10^-10 xray

Select the correct statement for energy level n=9 A) Each of the d orbitals have different energy B) All three p orbitals have the same energy because they are degenerate C) The two s orbitals have the same energy because they are degenerate D) There are a total of 81 electrons at n=9

All three p orbitals have the same energy because they are degenerate

Select the correct statement. a)Na+ and K+,are isoelectronic because they both lost one electron and are in Group 1A. b)Ar and K+ are isoelectronic because they both have 18 electrons. c)Na and Mg are isoelectronic because they both are in the third period. d)Ca+ and Ca2+ are isoelectronic because they both are charged atoms of calcium and lost electrons

Ar and K+ are isoelectronic because they both have 18 electrons

Which of the following electron configurations is correct? a)Ga: [Kr]4s23d104p1 b)Mo: [Kr]5s24d5 c)Ca: [Ar]4s13d10 d)Br: [Ar]4s23d104p5

Br

Rank the following in order of electron affinity: Mn KGeBr a) K > Mn > Ge > Br b) Br > Ge > K > Mn c) Br > Ge > Mn > K d) K > Ge > Mn > Br

Br > Ge > Mn > K

Which of the following compounds (or ions) contains an atom that does NOT follow the octet rule? a) BrF3 b) CBr4 c) NO+ d) BF4-

BrF3

Which of the following arrangements is in order of increasing size? a)Ca2+ > K+ > Cl- > S2- b)Ca2+ < K+ < Cl- < S2- c)S2- > Cl- > Ca2+ > K+ d)S2- < Cl- < K+ < Ca2+

Ca2+ < K+ < Cl- < S2-

Which of the following contains the most lattice energy? a) KCl b) BaCl2 c) CaS d)Na2O

CaS

energy is proportional to frequency:

E = hv

Order the elements S, Cl, and F in terms of decreasing ionization energy. a)S, Cl, F b) Cl, F, S c) F, S, Cl d) F, Cl, S

F, Cl, S

Order the elements S, Cl, and F in terms of increasing atomic radii. a) F, Cl, Sb) Cl, F, Sc) F, S, Cld) S, Cl, F

F, Cl, S

Which of the following bonds is least polar? a) C—O b) H—C c) P—Cl d) Na—Cl

H-C

A valid Lewis structure of ________ cannot be drawn without violating the octet rule. a) NI3 b) SO2 c) ICl5 d) SiF4

ICl5

Select the correct statements below. I. An atom of chlorine is larger than sulfur because the addition of an electron increases the repulsions without an increase in attraction for the nucleus resulting in less screening. II. An atom of oxygen is smaller than an atom of carbon because the distance of the valence electrons remains the same while the attraction for the nucleus increases with increasing number of protons. III. An atom of potassium is smaller than an atom of rubidium because size increases as the principal quantum number increases IV. An atom of sodium is smaller than an atom of magnesium because size decreases as the principal quantum number increases V. An atom of chlorine is smaller than an atom of bromine because the principal quantum number of the valence orbitals increases. VI. An atom of silicon is smaller than an atom of carbon because the principal quantum number of the valence orbitals increases

II, III, V

Which of the following statements is (are) true? I.Energy is directly proportional to wavelength. II. The energy of an atom is increased when electromagnetic radiation is emittedfrom it. III. The energy of electromagnetic radiation increases as its frequency increases. IV. An electron in the n = 4 state in the hydrogen atom can go to the n = 2 state by emitting electromagnetic radiation at the appropriate frequency. V.The frequency and wavelength of electromagnetic radiation are inversely proportional to each other.

III, IV, V

Select the correct statement a) Ionization energy and metallic character have the same trend. b) Ionization energy and atomic size have the same trend. c)Electron affinity and atomic size have the same trend. d)Ionization energy and electron affinity have the same trend

Ionization energy and electron affinity have the same trend

Select which of the following are correctly identified. a) Both CO and KBr are polar covalent molecules. b)Both MgO and HCl are ionic compounds. c)KBr is an ionic compound and I2 is a nonpolar covalent molecule. d)CO and H2 are nonpolar covalent molecules

KBr is an ionic compound and I2 is a nonpolar covalent molecule

In which group do all the elements have similar chemical properties? a) P, S, Cl b) Ag, Cd, Ar c) Na, Ca, Ba d) N, P, As e) none

N, P, As

Which of the following would have the greatest dipole? a) Cl—Br b) N—F c) O—F d) P—S

N-F

There can be two equivalent best resonance structures of ________. a) NO2- b) NO3- c) SO32- d) SO42-

NO2-

The atom with the highest second ionization energy is ________. a) Na b) Mg c) Al d) S

Na

The atom that has the most electron affinity is _______. a) Na b) Mg c) Al d) S

S

Select the correct statement below: a)Phosphorous contains 10 core electrons and 5 valence electrons. Its orbital diagram contains one half-filled 3p orbital and two filled 3p orbitals. b)Aluminum contains 10 core electrons and 3 valence electrons. Its orbital diagram contains three half-filled 3p orbitals. c)Calcium contains 18 core electrons and 2 valence electrons. Its orbital diagram contains two half-filled 4s orbitals and no filled 4p orbitals. d)Sodium contains 10 core electrons and 1 valence electron. Its orbital diagram contains one half-filled 3s orbital and three empty 3p orbitals

Sodium contains 10 core electrons and 1 valence electron. Its orbital diagram contains one half-filled 3s orbital and three empty 3p orbitals

Rank the following types of electromagnetic radiation in order of decreasing energy. a)X-rays > Ultraviolet > Visible > Microwaves b)Microwaves > Visible > Ultraviolet > X-rays c)Microwaves > Ultraviolet > Visible > X-rays d)X-rays > Visible > Ultraviolet > Microwaves

X-rays > Ultraviolet > Visible > Microwaves

Select the correct electron configuration of Fe A)[Ar]4s2 3d6 B) [Ar]4s2 4d6 C) [Ar] 3d6 D) [Ar] 4d6

a

In emission, ______. a)an electron moves from an excited state to a lower energy state, and energy is released. b)an electron moves from an excited state to a lower energy state, and energy is absorbed. c)an electron moves from a lower energy state to an excited state, and energy is released. d)an electron moves from a lower energy state to an excited state, and energy is absorbed

an electron moves from an excited state to a lower energy state, and energy is released

Select the correct electron configuration of Co3+ A)[Ar]4s2 3d7 B) [Ar]4s2 3d4 C) [Ar] 3d6 D) [Kr] 4s2 3d4

c

The electron pair in a H-F bond could be considered a)closer to H because hydrogen has a larger radius and thus exerts greater control over the shared electron pair b)closer to F because fluorine has a higher electronegativity than hydrogen c)closer to H because hydrogen has a lower electronegativity than fluorine

closer to F because fluorine has a higher electronegativity than hydrogen

centimeter

cm 10^-2 microwave

orbitals with the same value of n form an

electron shell

positive (triangle E) means

energy is absorbed

negative (triangle E) means

energy is released

electrons are in a higher energy state

excited state

electrons are in the lowest energy state

ground state

the values of n are

integers >_ 1

allowed values of I are

integers ranging from 0 to n-1

kilometer

km 1000 radio

The second ionization energy of Mg is 1445 kJ/mol. The first ionization energy is a)1445 kJ/mol b)less than 1445 kJ/mol c)greater than 1445 kJ/mol d)More information is needed to answer this question. e)None of these

less than 1445 kJ/mol

meter

m 1 television, radio

millimeter

mm 10^-3 microwave

The quantum numbers of the last electron of nickel could be: a) n = 3, ℓ = 2, mℓ = 0, ms = 1/2 b) n = 4, ℓ = 2, mℓ = 0, ms = 1/2 c) n = 3, ℓ = 1, mℓ = 0, ms = 1/2 d) n = 3, ℓ = 2, mℓ = 0, ms = 0

n=3, l=2, ml=0, ms=1/2

electron

negative charge, no mass

nanometer

nm 10^-9 unltraviolet, visible

neutron

no charge, mass

a specific designation within a subshell and refers to the number of values of mI for a given energy level (n)

orbital

energy released in a quanta of light is called a

photon

proton

positive charge, mass

Which of the following forms of electromagnetic radiation has the longest wavelength? a) microwaves b) ultraviolet c) infrared d) radio-waves

radio-waves

continuous spectrum

rainbow

Breaking bonds _____, while forming bonds _____. a) requires no energy; requires no energy b) releases energy; requires energy c) releases energy; releases energy d) requires energy; releases energy

requires energy; releases energy

Of the following elements, which is most likely to form a negative ion with charge 2-? a)Ba b)Ca c)S d)P e)Cl

s

combine n and I

subshells

Lattice energy is ____. a)the energy required to form one mole of an ionic compound from its ions in their gaseous states b)the energy required to break apart one mole of an ionic compound into its gaseous ions c)the energy required to remove an electron from an atom or ion in its gaseous state d)the energy required to add an electron to an atom or ion in its gaseous state

the energy required to break apart one mole of an ionic compound into its gaseous ions

An atomic orbital is defined by _____. a)the first three quantum numbers (n, l, ml) b)the principle quantum number only (n) c)all four quantum numbers (n, l, ml, ms) d)the first two quantum numbers (n, l)

the first three quantum numbers

An element with the electron configuration [Xe] 6s14f145d9 would belong to which class on the periodic table? a)rare earth elements b)alkaline earth elements c)halogens d)transition elements

transition elements

micrometer

um 10^-6 infrared