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Georgia State University - CHEM 1211Kpractice exam 3

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Exam

Name___________________________________

 

 

MULTIPLE CHOICE.  Choose the one alternative that best completes the statement or answers the question.

 

1)
 

 

On the electromagnetic spectrum, visible light is immediately between two other wavelengths.  Name them.
 

 

1)
 

 

_______

 

A)
 

 

infrared and ultraviolet

 

B)
 

 

microwave and x-ray

 

C)
 

 

gamma ray and ultraviolet

 

D)
 

 

infrared and x-ray

 

E)
 

 

radio and microwave

 

 

 

2)
 

 

Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.
 

 

2)
 

 

_______

 

A)
 

 

436 nm
 

 

B)
 

 

675 nm
 

 

C)
 

 

229 nm
 

 

D)
 

 

485 nm
 

 

E)
 

 

206 nm

 

 

 

3)
 

 

Which of the following occur as the energy of a photon increases?
 

 

3)
 

 

_______

 

A)
 

 

the wavelength increases

 

B)
 

 

the wavelength gets shorter.

 

C)
 

 

the frequency decreases.

 

D)
 

 

the speed increases.

 

E)
 

 

None of the above occur as the energy of a photon increases.

 

 

 

4)
 

 

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal, if the binding energy for an electron in K is 1.76 × 103 kJ/mol.
 

 

4)
 

 

_______

 

A)
 

 

147 nm
 

 

B)
 

 

885 nm
 

 

C)
 

 

68.0 nm
 

 

D)
 

 

387 nm
 

 

E)
 

 

113 nm

 

 

 

5)
 

 

Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s.
 

 

5)
 

 

_______

 

A)
 

 

5.52 × 10-9 m

 

B)
 

 

5.03 × 10-10 m

 

C)
 

 

1.81 × 10-10 m

 

D)
 

 

1.99 × 10-10 m

 

E)
 

 

2.76 × 10-9 m

 

 

 

6)
 

 

For n = 3, what are the possible sublevels?
 

 

6)
 

 

_______

 

A)
 

 

0, 1
 

 

B)
 

 

0, 1, 2, 3
 

 

C)
 

 

0, 1, 2
 

 

D)
 

 

0

 

 

 

7)
 

 

What are the possible orbitals for n = 3?
 

 

7)
 

 

_______

 

A)
 

 

s, p, d, f
 

 

B)
 

 

s, p
 

 

C)
 

 

s, p, d
 

 

D)
 

 

s

 

 

 

8)
 

 

Which of the following statements is TRUE?
 

 

8)
 

 

_______

 

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)
 

 

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

 

D)
 

 

Since electrons have mass, we must always consider them to have particle properties and never wavelike properties.

 

E)
 

 

All of the above are true.

 

 

 

9)
 

 

Which of the following quantum numbers describes the shape of an orbital?
 

 

9)
 

 

_______

 

A)
 

 

Schrödinger quantum number

 

B)
 

 

angular momentum quantum number

 

C)
 

 

principal quantum number

 

D)
 

 

spin quantum number

 

E)
 

 

magnetic quantum number

 

 

 

10)
 

 

Which of the following quantum numbers describes the orientation of an orbital?
 

 

10)
 

 

______

 

A)
 

 

spin quantum number

 

B)
 

 

 Schrödinger quantum number

 

C)
 

 

magnetic quantum number

 

D)
 

 

principal quantum number

 

E)
 

 

angular momentum quantum number

 

 

 

11)
 

 

Which of the following quantum numbers describes the size and energy of an orbital?
 

 

11)
 

 

______

 

A)
 

 

magnetic quantum number

 

B)
 

 

spin quantum number

 

C)
 

 

 Schrödinger quantum number

 

D)
 

 

angular momentum quantum number

 

E)
 

 

principal quantum number

 

 

 

12)
 

 

If two electrons in the same atom have the same value of "l", they are
 

 

12)
 

 

______

 

A)
 

 

in the same level, but different sublevel.

 

B)
 

 

in the same sublevel, but not necessarily in the same level.

 

C)
 

 

in different levels and in different shaped orbitals.

 

D)
 

 

in the same orbital.

 

E)
 

 

none of the above.

 

 

 

13)
 

 

Describe the shape of a p orbital.
 

 

13)
 

 

______

 

A)
 

 

three balls

 

B)
 

 

spherical

 

C)
 

 

eight balls

 

D)
 

 

dumbbell shaped

 

E)
 

 

four balls

 

 

 

14)
 

 

Give the numbers for ml for an f orbital.
 

 

14)
 

 

______

 

A)
 

 

-3, -2, -1, 0, 1, 2, 3
 

 

B)
 

 

0, 1, 2, 3

 

C)
 

 

1, 2, 3, 4
 

 

D)
 

 

-2, -1, 0, 1, 2

 

 

 

15)
 

 

No two electrons can have the same four quantum numbers is known as the
 

 

15)
 

 

______

 

A)
 

 

Heisenberg uncertainty principle
 

 

B)
 

 

Pauli exclusion principle

 

C)
 

 

Hund's rule
 

 

D)
 

 

Aufbau principle

 

 

 

16)
 

 

Only two electrons, with opposing spins, are allowed in each orbital is known as the
 

 

16)
 

 

______

 

A)
 

 

Hund's rule
 

 

B)
 

 

Aufbau principle

 

C)
 

 

Heisenberg uncertainty principle
 

 

D)
 

 

Pauli exclusion principle

 

 

 

17)
 

 

Choose the orbital diagram that represents the ground state of N.
 

 

17)
 

 

______

 

A)
 

 

 

 

 

B)
 

 

 

 

 

C)
 

 

 

 

 

D)
 

 

 

 

 

E)
 

 

 

 

 

 

 

18)
 

 

What period 3 element having the following ionization energies (all in kJ/mol)?

 

IE1 = 1012        IE2 = 1900    IE3= 2910     IE4= 4960     IE5= 6270     IE6 = 22,200

 
 

 

18)
 

 

______

 

A)
 

 

P
 

 

B)
 

 

Mg
 

 

C)
 

 

Si
 

 

D)
 

 

Cl
 

 

E)
 

 

S

 

 

 

19)
 

 

Place the following in order of increasing IE1.

 

                N                F                  As

 
 

 

19)
 

 

______

 

A)
 

 

As  <  N  <  F

 

B)
 

 

As  <  F  <  N

 

C)
 

 

N  <  As  <  F

 

D)
 

 

F  <  N  <  As

 

E)
 

 

F  <  As  <  N

 

 

 

20)
 

 

Identify the species that has the smallest radius.
 

 

20)
 

 

______

 

A)
 

 

anion
 

 

B)
 

 

neutral

 

C)
 

 

cation
 

 

D)
 

 

they are all the same size

 

 

 

21)
 

 

Identify the number of valence electrons in Cl-1.
 

 

21)
 

 

______

 

A)
 

 

8
 

 

B)
 

 

4
 

 

C)
 

 

7
 

 

D)
 

 

5
 

 

E)
 

 

6

 

 

 

22)
 

 

Give the ground state electron configuration for Br⁻.
 

 

22)
 

 

______

 

A)
 

 

[Ar]4s24p6

 

B)
 

 

[Ar]4s23d104p5

 

C)
 

 

[Ar]4s23d104p6

 

D)
 

 

[Ar]4s23d104p4

 

E)
 

 

[Ar]4s24d104p6

 

 

 

23)
 

 

Which of the following represent the Lewis structure for Cl?
 

 

23)
 

 

______

 

A)
 

 

 
 

 

B)
 

 

 
 

 

C)
 

 

 
 

 

D)
 

 

 
 

 

E)
 

 

 

 

 

 

24)
 

 

Give the complete electronic configuration for Br-.
 

 

24)
 

 

______

 

A)
 

 

1s22s22p63s23p64s24d104p6

 

B)
 

 

1s22s22p63s23p64s24p6

 

C)
 

 

1s22s22p63s23p64s23d104p5

 

D)
 

 

1s22s2p63s2p64s23d104p6

 

E)
 

 

1s22s22p63s23p64s23d104p6

 

 

 

25)
 

 

Which of the following statements is TRUE?
 

 

25)
 

 

______

 

A)
 

 

An ionic bond is much stronger than most covalent bonds.

 

B)
 

 

Once dissolved in water, ionic compounds rarely conduct electricity.

 

C)
 

 

Ionic compounds at room temperature typically conduct electricity.

 

D)
 

 

An ionic bond is formed through the sharing of electrons.

 

E)
 

 

None of the above are true.

 

 

 

26)
 

 

Use Lewis theory to determine the chemical formula for the compound formed between Al and O.
 

 

26)
 

 

______

 

A)
 

 

Al3O2
 

 

B)
 

 

Al2O3
 

 

C)
 

 

AlO
 

 

D)
 

 

AlO2
 

 

E)
 

 

Al2O

 

 

 

27)
 

 

A single covalent bond contains ________ of electrons.
 

 

27)
 

 

______

 

A)
 

 

1 pair
 

 

B)
 

 

3 pairs
 

 

C)
 

 

0 pairs
 

 

D)
 

 

2 pairs
 

 

E)
 

 

4 pairs

 

 

 

28)
 

 

Identify the shortest bond.
 

 

28)
 

 

______

 

A)
 

 

triple covalent bond

 

B)
 

 

double covalent bond

 

C)
 

 

single covalent bond

 

D)
 

 

all of the above bonds are the same length

 

 

 

29)
 

 

Identify the number of bonding pairs and lone pairs of electrons in water.
 

 

29)
 

 

______

 

A)
 

 

2 bonding pairs and 1 lone pair

 

B)
 

 

2 bonding pairs and 2 lone pairs

 

C)
 

 

3 bonding pairs and 2 lone pairs

 

D)
 

 

1 bonding pair and 1 lone pair

 

E)
 

 

1 bonding pair and 2 lone pairs

 

 

 

30)
 

 

Identify the compound with the smallest dipole moment in the gas phase.
 

 

30)
 

 

______

 

A)
 

 

HF
 

 

B)
 

 

ClF
 

 

C)
 

 

LiF
 

 

D)
 

 

Cl2

 

 

 

31)
 

 

Choose the best Lewis structure for OCl2.
 

 

31)
 

 

______

 

A)
 

 

 

 

B)
 

 

 

 

C)
 

 

 

 

D)
 

 

 

 

E)
 

 

 

 

 

 

32)
 

 

Give the number of valence electrons for XeI2.
 

 

32)
 

 

______

 

A)
 

 

18
 

 

B)
 

 

16
 

 

C)
 

 

20
 

 

D)
 

 

22
 

 

E)
 

 

24

 

 

 

33)
 

 

Choose the best Lewis structure for SO42⁻.
 

 

33)
 

 

______

 

A)
 

 

 

 

 

B)
 

 

 

 

 

C)
 

 

 

 

 

D)
 

 

 

 

 

E)
 

 

 

 

 

 

 

34)
 

 

Draw the Lewis structure for CO32- including any valid resonance structures.  Which of the following statements is TRUE?
 

 

34)
 

 

______

 

A)
 

 

The CO32- ion contains two C—O single bonds and one CO triple bond.

 

B)
 

 

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

 

C)
 

 

The CO32- ion contains three C—O double bonds.

 

D)
 

 

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

 

E)
 

 

None of the above are true.

 

 

 

35)
 

 

Using Lewis structures and formal charge, which of the following ions is most stable?

 

                OCN⁻         ONC⁻        NOC⁻

 
 

 

35)
 

 

______

 

A)
 

 

ONC⁻

 

B)
 

 

NOC⁻

 

C)
 

 

OCN⁻

 

D)
 

 

None of these ions are stable according to Lewis theory.

 

E)
 

 

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

 

 

 

36)
 

 

Place the following in order of increasing  bond length.

 

                NO2⁻         NO3⁻         NO

 
 

 

36)
 

 

______

 

A)
 

 

NO3⁻  <  NO2⁻  <  NO

 

B)
 

 

NO  <  NO2⁻  <  NO3⁻

 

C)
 

 

NO2⁻  <  NO3⁻  <  NO

 

D)
 

 

NO  <  NO3⁻  <  NO2⁻

 

E)
 

 

NO3⁻  <  NO <  NO2⁻

 

 

 

37)
 

 

Use the bond energies provided to estimate ΔH°rxn for the reaction below.

 

                                PCl3(g) + Cl2(g)  →  PCl5(l)            ΔH°rxn = ?

Bond              Bond Energy (kJ/mol)

Cl-Cl              243

P-Cl                331

 
 

 

37)
 

 

______

 

A)
 

 

-662 kJ
 

 

B)
 

 

-243 kJ
 

 

C)
 

 

-67 kJ
 

 

D)
 

 

-905 kJ
 

 

E)
 

 

-419 kJ

 

 

 

38)
 

 

Determine the electron geometry (eg) and molecular geometry(mg) of BCl3.
 

 

38)
 

 

______

 

A)
 

 

eg=trigonal planar, mg=trigonal planar

 

B)
 

 

eg=tetrahedral, mg=trigonal planar

 

C)
 

 

eg=trigonal planar, mg=bent

 

D)
 

 

eg=trigonal bipyramidal, mg= trigonal bipyramidal

 

E)
 

 

eg=tetrahedral, mg=trigonal pyramidal

 

 

 

39)
 

 

Consider the molecule below.  Determine the molecular geometry at each of the 3 labeled atoms.

 

 
 

 

39)
 

 

______

 

A)
 

 

1=trigonal planar, 2=tetrahedral, 3=trigonal pyramidal

 

B)
 

 

1=tetrahedral, 2=tetrahedral, 3=tetrahedral

 

C)
 

 

1=tetrahedral, 2=tetrahedral, 3=trigonal planar

 

D)
 

 

1=trigonal planar, 2=trigonal pyramidal, 3=trigonal pyramidal

 

E)
 

 

1=trigonal planar, 2=tetrahedral, 3=tetrahedral

 

 

 

40)
 

 

Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule.

 

                PF3             OF2            PF4⁺

 
 

 

40)
 

 

______

 

A)
 

 

OF2  <  PF4⁺  <  PF3

 

B)
 

 

PF4⁺  < PF3  <  OF2

 

C)
 

 

OF2  <  PF3  <  PF4⁺

 

D)
 

 

PF4⁺  <  OF2  <  PF3

 

E)
 

 

PF3  <  OF2  <  PF4⁺

 

 

 

41)
 

 

Place the following in order of increasing dipole moment.

 

                I.  BCl3                   II.  BIF2                  III.  BClF2

 
 

 

41)
 

 

______

 

A)
 

 

II <  I  <  III

 

B)
 

 

I <  III  <  II

 

C)
 

 

II <  III <  I

 

D)
 

 

I <  II  <  III

 

E)
 

 

I <  II = III

 

 

 

42)
 

 

Identify the number of electron groups around a molecule with sp hybridization.
 

 

42)
 

 

______

 

A)
 

 

5
 

 

B)
 

 

3
 

 

C)
 

 

1
 

 

D)
 

 

4
 

 

E)
 

 

2

 

 

 

43)
 

 

Identify the number of electron groups around a molecule with sp2 hybridization.
 

 

43)
 

 

______

 

A)
 

 

5
 

 

B)
 

 

3
 

 

C)
 

 

4
 

 

D)
 

 

1
 

 

E)
 

 

2

 

 

 

44)
 

 

Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O.
 

 

44)
 

 

______

 

A)
 

 

eg=trigonal pyramidal, mg=trigonal pyramidal, sp3

 

B)
 

 

eg=tetrahedral, mg=bent, sp3

 

C)
 

 

eg=trigonal planar, mg=trigonal planar, sp2

 

D)
 

 

eg=tetrahedral, mg=trigonal pyramidal, sp3

 

E)
 

 

eg=bent, mg=bent, sp2

 

 

 

45)
 

 

Give the hybridization for the Br in BrO4⁻. 
 

 

45)
 

 

______

 

A)
 

 

sp3d2
 

 

B)
 

 

sp
 

 

C)
 

 

sp3d
 

 

D)
 

 

sp3
 

 

E)
 

 

sp2

 

 

 

46)
 

 

Give the hybridization for the S in SF6.  
 

 

46)
 

 

______

 

A)
 

 

sp
 

 

B)
 

 

sp3d
 

 

C)
 

 

sp3
 

 

D)
 

 

sp2
 

 

E)
 

 

sp3d2


 

 

 

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[Solved] Georgia State University - CHEM 1211Kpractice exam 3

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Exam Name___________________________________ MULTIPLE CHOICE.  Choose the one alternative that best completes the statement or answers the question. 1) On the electromagnetic spectrum, visible light is immediately between two other wavelengths.  Name them. 1) _______ A) infrared and ultraviolet B) microwave and x-ray C) gamma ray and ultraviolet D) infrared and x-ray E) radio and microwave 2) Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz. 2) _______ A) 436 nm B) 675 nm C) 229 nm D) 485 nm E) 206 nm 3) Which of the following occur as the energy of a photon increases? 3) _______ A) the wavelength increases B) the wavelength gets shorter. C) the frequency decreases. D) the speed increases. E) None of the above occur as the energy of a photon increases. 4) Determine the longest wavelength of light required to remove an electron from a sample of potassium metal, if the binding energy for an electron in K is 1.76 × 103 kJ/mol. 4) _______ A) 147 nm B) 885 nm C) 68.0 nm D) 387 nm E) 113 nm 5) Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s. 5) _______ A) 5.52 × 10-9 m B) 5.03 × 10-10 m C) 1.81 × 10-10 m D) 1.99 × 10-10 m E) 2.76 × 10-9 m 6) For n = 3, what are the possible sublevels? 6) _______ A) 0, 1 B) 0, 1, 2, 3 C) 0, 1, 2 D) 0 7) What are the possible orbitals for n = 3? 7) _______ A) s, p, d, f B) s, p C) s, p, d D) s 8) Which of the following statements is TRUE? 8) _______ 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) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. D) Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. E) All of the above are true. 9) Which of the following quantum numbers describes the shape of an orbital? 9) _______ A) Schrödinger quantum number B) angular momentum quantum number C) principal quantum number D) spin quantum number E) magnetic quantum number 10) Which of the following quantum numbers describes the orientation of an orbital? 10) ______ A) spin quantum number B)  Schrödinger quantum number C) magnetic quantum number D) principal quantum number E) angular momentum quantum number 11) Which of the following quantum numbers describes the size and energy of an orbital? 11) ______ A) magnetic quantum number B) spin quantum number C)  Schrödinger quantum number D) angula...
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