CHM151 Chapters 7-9

Identify the element that has a ground state electronic configuration of [Kr]5s24d5. A) Tc B) Mn C) Nb D) Ru

A) Tc

Halogens can react with each other to form A) covalent bonds. B) ionic bonds. C) salts. D) hydrogen halides. E) metal halides.

A) covalent bonds.

Identify the elements correctly shown by decreasing radii size. A) N3- > N B) K+ > K C) N > N3- D) Cu2+ > Cu+ E) S- > S2-

B) K+ > K C) N > N3- D) Cu2+ > Cu+ E) S- > S2-

Choose the best Lewis structure for BeF2. A) B) C) D) E)

D)

Choose the best Lewis structure for ICl5. A) B) C) D) E)

D)

Choose the valence orbital diagram that represents the ground state of Sr2⁺. A) B) C) D)

D)

Which of the following represents the Lewis structure for Br⁻? A) B) C) D) E)

D)

How many valence electrons do the halogens possess? A) 5 B) 6 C) 2 D) 1 E) 7

E) 7

Choose the valence orbital diagram that represents the ground state of Zn. A) B) C) D) E)

A)

Which of the following represents the Lewis structure for S2⁻? A) B) C) D) E)

A)

Draw the best Lewis structure for Cl3⁻. What is the formal charge on the central Cl atom? A) -1 B) 0 C) +1 D) +2 E) -2

A) -1

How many valence electrons do the alkali metals possess? A) 1 B) 2 C) 7 D) 6 E) 8

A) 1

24) The Lewis structure of sulfuric acid contains A) 2 double bonds, 4 single bonds, and 8 lone pairs. B) 4 double bonds, and two single bonds. C) 2 double bonds and 4 single bonds. D) 6 single bonds and 4 lone pairs. E) 2 double bonds, 4 single bonds, and 4 lone pairs.

A) 2 double bonds, 4 single bonds, and 8 lone pairs.

Give the number of valence electrons for SO42-. A) 32 B) 30 C) 34 D) 28 E) 36

A) 32

Which of the following statements is TRUE? A) An ionic bond is much stronger than most covalent bonds. B) An ionic bond is formed through the sharing of electrons. C) Ionic compounds at room temperature typically conduct electricity. D) Once dissolved in water, ionic compounds rarely conduct electricity. E) None of the above is true.

A) An ionic bond is much stronger than most covalent bonds.

Identify the most reactive alkali metal with water. A) Cs B) Rb C) K D) Na E) Li

A) Cs

Which reaction below represents the electron affinity of Li? A) Li(g) + e⁻ → Li⁻(g) B) Li(g) → Li⁺(g) + e⁻ C) Li(g) + e⁻ → Li⁺(g) D) Li⁺(g) → Li(g) + e⁻ E) Li⁺(g) + e⁻ → Li(g)

A) Li(g) + e⁻ → Li⁻(g)

Place the following in order of increasing magnitude of lattice energy. CaO MgO SrS A) MgO < CaO < SrS B) SrS < MgO < CaO C) SrS < CaO < MgO D) CaO < MgO < SrS E) CaO < SrS < MgO

A) MgO < CaO < SrS

No two electrons can have the same four quantum numbers is known as (the) A) Pauli exclusion principle. B) Hund's rule. C) Aufbau principle. D) Heisenberg uncertainty principle.

A) Pauli exclusion principle.

When waves of equal amplitude from two sources are out of phase when they interact, it is called A) destructive interference. B) diffraction. C) constructive interference. D) effusion. E) amplitude.

A) destructive interference.

Describe the reaction of the noble gases with metals. A) inert B) vigorous C) mild reaction D) forms water E) dissolves

A) inert

A cation of +2 indicates that an element has A) lost two electrons. B) lost two protons. C) lost two neutrons. D) gained two electrons. E) gained two protons.

A) lost two electrons.

Which of the following quantum numbers describes the orientation of an orbital? A) magnetic quantum number B) principal quantum number C) angular momentum quantum number D) spin quantum number E) Schrödinger quantum number

A) magnetic quantum number

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Cl atom. A) n = 3, l = 1, ml = 1, ms = +1/2 B) n = 3, l = 0, ml = 1, ms = +1/2 C) n = 3, l = 2, ml =1, ms = -1/2 D) n = 2, l = 1, ml = 1, ms = +1/2 E) n = 3, l =1, ml = 1, ms = -1/2

A) n = 3, l = 1, ml = 1, ms = +1/2

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Sr atom. A) n = 5, l = 0, ml = 0, ms = -1/2 B) n = 4, l = 1, ml = -1 ms = -1/2 C) n = 5, l = 0, ml = 0, ms = +1/2 D) n = 4, l = 1, ml = -1, ms = +1/2 E) n = 5, l = 1, ml =1, ms = -1/2

A) n = 5, l = 0, ml = 0, ms = -1/2

A sunburn is caused by overexposure to ________ radiation. A) ultraviolet B) gamma C) microwave D) x-ray E) radio

A) ultraviolet

Identify the color of a flame test for potassium. A) violet B) red C) white D) yellow E) blue

A) violet

A reaction is exothermic when A) weak bonds break and strong bonds form. B) strong bonds break and weak bonds form. C) weak bonds break and weak bonds form. D) strong bonds break and strong bonds form.

A) weak bonds break and strong bonds form.

Choose the best Lewis structure for BF3. A) B) C) D) E)

B)

Choose the best Lewis structure for CH2Cl2. A) B) C) D) E)

B)

Choose the best Lewis structure for XeI2. A) B) C) D) E)

B)

Which of the following represents the Lewis structure for Cl? A) B) C) D) E)

B)

Use the data given below to construct a Born-Haber cycle to determine the electron affinity of Br. DH°(kJ) K(s) → K(g) 89 K(g) → K⁺(g) + e⁻ 419 Br2(l) → 2 Br(g) 193 K(s) + Br2(g) → KBr(s) -394 KBr(s) → K⁺(g) + Br⁻(g) 674 A) -885 kJ B) -325 kJ C) +367 kJ D) -464 kJ E) +246 kJ

B) -325 kJ

Calculate the wavelength of a baseball (m = 155 g) moving at 32.5 A) 7.60 × 10-36 m B) 1.32 × 10-34 m C) 2.15 × 10-32 m D) 2.68 × 10-34 m E) 3.57 × 10-32 m

B) 1.32 × 10-34 m

Give the complete electronic configuration for Ca2+. A) 1s22s22p63s24p6 B) 1s22s22p63s23p6 C) 1s22s22p63s23p5 D) 1s22s23p64s25p6 E) 1s22s2p63s2p6

B) 1s22s22p63s23p6

Give the complete electronic configuration for oxygen. A) 1s22s22py22pz2 B) 1s22s22px22py12pz1 C) 1s22s22px22pz2 D) 1s22s22px22py2 E) 1s22s22px4

B) 1s22s22px22py12pz1

What value of l is represented by a d orbital? A) 1 B) 2 C) 0 D) 3

B) 2

Draw the Lewis structure for CO32- including any valid resonance structures. Which of the following statements is TRUE? A) The CO32- ion contains one C-O single bond and two CO double bonds. B) The CO32- ion contains two C-O single bonds and one CO double bond. C) The CO32- ion contains three C-O double bonds. D) The CO32- ion contains two C-O single bonds and one CO triple bond. E) None of the above is true.

B) The CO32- ion contains two C-O single bonds and one CO double bond.

Choose the ground state electron configuration for Zn2⁺. A) [Ar]4s23d8 B) [Ar]3d10 C) [Ar]4s23d6 D) [Ar] E) [Ar]3d8

B) [Ar]3d10

When a wave encounters an obstacle or a slit that is comparable in size to its wavelength, it bends around it. This characteristic is called A) destructive interference. B) diffraction. C) constructive interference. D) effusion. E) amplitude.

B) diffraction.

Identify the color of a flame test for lithium. A) violet B) red C) white D) yellow E) blue

B) red

Choose the best Lewis structure for PO43⁻. A) B) C) D) E)

C)

For n = 3, what are the possible values for l? A) 0 B) 0, 1 C) 0, 1, 2 D) 0, 1, 2, 3

C) 0, 1, 2

Determine the mass of a ball with a wavelength of 3.45 × 10-34 m and a velocity of 6.55 m/s. A) 0.293 g B) 12.6 g C) 293 g D) 346 g E) 3.41 g

C) 293 g

Calculate the energy of the orange light emitted, per photon, by a neon sign with a frequency of 4.89 × 1014 Hz. A) 3.09 × 10-19 J B) 6.14 × 10-19 J C) 3.24 × 10-19 J D) 1.63 × 10-19 J E) 5.11 × 10-19 J

C) 3.24 × 10-19 J

Place the following in order of decreasing IE1. Cs Mg Ar A) Cs > Mg > Ar B) Mg > Ar > Cs C) Ar > Mg > Cs D) Cs > Ar > Mg E) Mg > Cs > Ar

C) Ar > Mg > Cs

When filling degenerate orbitals, electrons fill them singly first, with parallel spins. This is known as (the) A) Pauli exclusion principle. B) Hund's rule. C) Aufbau principle. D) Heisenberg uncertainty principle.

C) Aufbau principle.

Place the following in order of decreasing magnitude of lattice energy. K2O Rb2S Li2O A) Li2O > K2O > Rb2S B) Li2O > Rb2S > K2O C) Rb2S > K2O > Li2O D) Rb2S > Li2O > K2O E) K2O > Li2O > Rb2S

C) Rb2S > K2O > Li2O

Give the ground state electron configuration for Sr. A) [Kr]5s24d2 B) [Kr]5s24d105p2 C) [Kr]5s2 D) [Kr]5s25d105p2 E) [Kr]5s24d10

C) [Kr]5s2

Which of the following visible colors of light has the highest frequency? A) green B) red C) blue D) yellow E) orange

C) blue

The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is A) titanium. B) vanadium. C) chromium. D) manganese. E) iron.

C) chromium.

The number of cycles that pass through a stationary point is called A) wavelength. B) amplitude. C) frequency. D) area. E) median.

C) frequency.

Food can be cooked by ________ radiation. A) ultraviolet B) gamma C) microwave D) x-ray E) radio

C) microwave

Which of the following colors of electromagnetic radiation has the shortest wavelength? A) blue B) violet C) orange D) green E) yellow

C) orange

Identify the shortest bond. A) single covalent bond B) double covalent bond C) triple covalent bond D) All of the above bonds are the same length.

C) triple covalent bond

When an electric current is passed through a tube containing helium, helium atoms absorb some of the electrical energy and reemit it as a ________ color. A) white B) yellow C) violet D) blue E) red

C) violet

How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy? A) 5.67 × 1023 photons B) 2.01 × 1024 photons C) 1.25 × 1031 photons D) 4.99 × 1023 photons E) 7.99 × 1030 photons

D) 4.99 × 1023 photons

Use the data given below to construct a Born-Haber cycle to determine the bond energy of O2. DH°(kJ) Na(s) → Na(g) 107 Na(g) → Na⁺(g) + e⁻ 496 O(g) + e⁻ → O⁻(g) -141 O⁻(g) + e⁻ → O2⁻(g) 878 2 Na(s) + O2(g) → Na2O(s) -416 2 Na⁺(g) + O2⁻(g) → Na2O(s) -2608 A) 426 kJ B) 249 kJ C) 852 kJ D) 498 kJ E) 356 kJ

D) 498 kJ

Which of the following statements is TRUE? A) We can sometimes know the exact location and speed of an electron at the same time. B) All orbitals in a given atom are roughly the same size. C) Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. E) All of the above are true.

D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape.

________, used to destroy molecules within unwanted cells such as cancer cells, are called ionizing radiation. A) Beta and gamma rays B) Alpha and beta rays C) Microwave and infrared D) X-rays and gamma rays E) Visible and microwave

D) X-rays and gamma rays

Identify the orbital. A) d orbital B) dxy orbital C) px orbital D) f orbital E) py orbital

D) f orbital

Choose the best Lewis structure for NH4⁺ A) B) C) D) E)

E)

What total energy (in kJ) is contained in 1.0 mol of photons, all with a frequency of 2.75 × 1014 Hz? A) 182 kJ B) 219 kJ C) 457 kJ D) 326 kJ E) 110 kJ

E) 110 kJ

Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm. A) 3.54 × 10-19 J B) 4.27 × 10-19 J C) 2.34 × 10-19 J D) 6.45 × 10-19 J E) 2.83 × 10-19 J

E) 2.83 × 10-19 J

Which of the following statements is TRUE? A) The emission spectrum of a particular element is always the same and can be used to identify the element. B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. C) The uncertainty principle states that we can never know both the exact location and speed of an electron. D) An orbital is the volume in which we are most likely to find an electron. E) All

E) All of the above are true.

Using Lewis structures and formal charge, which of the following ions is most stable,? OCN⁻ ONC⁻ NOC⁻ A) OCN⁻ B) ONC⁻ C) NOC⁻ D) None of these ions are stable according to Lewis theory. E) All of these compounds are equally stable according to Lewis theory.

E) All of these compounds are equally stable according to Lewis theory.

Which of the following statements is TRUE? A) A covalent bond is formed through the transfer of electrons from one atom to another. B) A pair of electrons involved in a covalent bond is sometimes referred to as a "lone pair." C) It is not possible for two atoms to share more than two electrons. D) Single bonds are shorter than double bonds. E) In a covalent bond, the shared electrons interact with the nuclei of both of the bonding atoms, thus lowering their potential energy.

E) In a covalent bond, the shared electrons interact with the nuclei of both of the bonding atoms, thus lowering their potential energy.

Place the following in order of decreasing metallic character. P As K A) P > As > K B) As > P > K C) K > P > As D) As > K > P E) K > As > P

E) K > As > P

What period 3 element has the following ionization energies (all in kJ/mol)? IE1 = 1012 IE2 = 1900 IE3 = 2910 IE4 = 4960 IE5 = 6270 IE6 = 22,200 A) Si B) S C) P D) Cl E) Mg

E) Mg

Identify the isoelectronic elements. A) Cl-, F-, Br-, I-, At- B) N3-, S2-, Br-, Cs+, Sr2+ C) P3-, S2-, C1-, K+, Ca2+ D) Zn2+, Co2+, Cu2+, Cr2+, Cd2+ E) Ne, Ar, Kr, Xe, He

E) Ne, Ar, Kr, Xe, He

Give the ground state electron configuration for Cd. A) [Kr]5s25d10 B) [Kr]5s24d105p2 C) [Kr]4d10 D) [Kr]5s24d8 E) [Kr]5s24d10

E) [Kr]5s24d10

Give the ground state electron configuration for the ion of Ba. A) [Kr]5s25p6 B) [Kr]5s24d105p66s26p2 C) [Kr]5s24d105p66s1 D) [Kr]5s24d105p66s2 E) [Kr]5s24d105p6

E) [Kr]5s24d105p6

A type of energy embodied in oscillating electric and magnetic fields is called A) infrared radiation. B) microwave radiation. C) magnetism. D) electricity. E) electromagnetic radiation.

E) electromagnetic radiation.

When an electric current is passed through a tube containing neon, neon atoms absorb some of the electrical energy and reemit it as a ________ color. A) white B) yellow C) violet D) blue E) red

E) red

Define electronegativity. A) the ability of an atom to repel neutrons in a chemical bond B) the ability of an atom to repel electrons in a chemical bond C) the ability of an atom to attract protons to itself in a chemical bond D) the ability of an atom to attract neutrons to itself in a chemical bond E) the ability of an atom to attract electrons to itself in a chemical bond

E) the ability of an atom to attract electrons to itself in a chemical bond