(Answered)-Hi can you answer the questions about 4 hours Final exam review - (2025 Updated Original AI-Free Solution

Question

1. Hi

can you answer the questions about 4 hours?

Final exam review Chem 1411 Spring 2015 This is only a review. You are responsible for all material covered in the course. ?

Prepared by

?Prof. Alka Shukla

Department of Natural Science

HCCS Northeast

1. ??????? Do the following calculations and write the best answer?

???????????????????????

(12.345 + 0.450 + 45.4)

(12.134 + 0.510 ) / 29.4

34.175 x (0.990 + 78.4)

??????????? ?

???????????????????????

2.???????? A) What is the mass of a 123.4 mL sample if density is 1.74 g/mL?

??????????? B) What is the volume of a 450 Kg sample if density is 0.94 g/mL?

??????????? ?

???????????????????????

3.???????? Write the strongest intermolecular interactions for each of the? following molecules and predict which one is likely to have highest boiling point.

??????????? A) ?????? CH3CH2 CH₂OH

B) ?????? CH₃CH₂O CH₂CH₃

C) ?????? CH₃CH₂?NH₂??

D) ?????? CH₃CH₂?CH₂CH₃

E) ?????? CH₃CH₂?CH₂Cl

???????????

4.???????? List the following is an example of a chemical change or physical change?

??????????? A)??????? water boiling

??????????? B)??????? Snow melting

??????????? C)??????? Hydrogen gas tank exploding

??????????? D)??????? Lake water evaporating during summer

??????????? E)??????? solid carbon di oxide ?vaporizing

F)??????? Candle burning

5.???????? Write the symbols the elements silver, Antimony, tin, chlorine, Sodium, ?phosphorus, potassium, arsenic? and sulfur .

???????????

6.???????? Write the formula of Sulfate ion, ?phosphate ion,? Chlorate ion, Bi sulfite ion, hydroxide ion, the nitrate ion. ?

???????????

7.???????? Write the formulae / names and molar mass of the following compounds????

A)??????? Potassium carbonate

??????????? B)??????? Barium sulfate

??????????? C)??????? Ammonium sulfate

??????????? D)??????? Copper( I) phosphate

??????????? E)??????? Chromium( IV) sulfide

??????????? F) FeCl₂

??????????? G) a compound formed between magnesium and nitrate ions.

??????????? H) a compound formed between potassium and sulfide ions.?

I) NH₄NO₃

8.???????? Calculate the number of moles in

23.45 g of Iron

56.45 g of Arsenic

9.???????? Write the empirical formula of

A) C₂H₆

B) C₃H₈

10.?????? Balance the following equations and sum the coefficients

???????????????????????

??????????? A)??????? ____ Na₃PO₄ + ____ KOH --->. ____ NaOH + ____ K₃PO₄

??????????? B)??????? ____ SO₂ + ____ Li₂Se --->. ____ SSe₂ + ____ Li₂O

?

??????????? E)??????? __ N₂H₄ + __ N₂O₄---->.? __ N₂ + __ H₂O

11.? At 50?C and 0.5? atm pressure, it is found that 3.24 L of gas weighs 1.11 g molar mass

??????????? is:

??????????? ?

???????????

12. Determine the empirical formula of a compound that is composed of 36.5% sodium, 25.4% sulfur, and 38.1% oxygen and molar mass was 378 g/mole

13.?????? Calculate the moles of? CO₂ produced when 3 moles of C₃H₈(g) reacts with 13 moles of O₂.

C₃H₈(g) + 5O₂(g) ? 3 CO₂(g) + 4H₂O(1)

????? ????? ?

14.?????? A 123.0-g sample of metal at 67.0?C is added to 150.0 g of H₂O at 25.0?C.? The temperature rises to

??????????? 24.3?C.? Assuming that the calorimeter is a perfect insulator, what is the specific heat of the metal??

??????????? (Specific heat of H₂O is 4.18 J/g ? ?C.)

??????????? ?

???????????

15.?????? Using the DH?_f following data, determine the heat of reaction for the combustion of

???????????????????????

???????????????????????????????????????????????????????????????????????

??????????? A)? ?C₂H₄(g) + 3O₂(g)--?? 2CO₂(g) + 2H₂O(1)

??????????? B)?? C₃H₈(g) + 5O₂(g) --? 3 CO₂(g) + 4H₂O(1)

??????????? ?

???????????

16.?????? According to the quantum theory, what is the energy contained in a single quantum with

??????????? a frequency of 5.67 ? 10^{14 s?1}?

???????????

17.?????? Which the name and symbol of quantum number describes the?

??????????? A)??????? orientation in space of an orbital???????

B)??????? Spin of electron

18. Perform the following conversions

56^oF to kelvin scale

145 K to ^oF????

23.6 miles to cm

5 ft 6 inches to cm

145 Lb to kg

???????????

19.?????? The maximum number of electrons that can occupy the

??????????? A)??????? 5f orbitals

??????????? B)??????? 4d orbitals??????

C)??????? 7 s orbitals

D)??????? 3p orbitals

4^th shell

3^rd shell

A single 3d orbital

???????????

20.?????? Which one of the following ?species will have chemical properties most similar to those of

???????????? The Nitrogen atoms??

A)??????? Oxygen atom

??????????? B)??????? fluorine atom

??????????? C)??????? nitride ?ion

??????????? D)??????? sulfide ion

??????????? E)??????? phosphorous atoms

21.?????? The elements having the electron configurations

??????????? A)??????? ns² np⁵ are called????????

B)??????? ns² called

??????????? C)??????? ns² np⁶ are called

???????????

22. Arrange in terms of largest to smallest radius.

??????????? A)??????? K, Al, S, As, Br

??????????? B)??????? C, Cl, N, S, Na

???????????

23.?????? What is the electron configuration of

??????????? A) Fe⁺³

_{?????????????????} B) Sn⁺²???????????

???????????

24.?????? What is the total number of valence electrons in the

??????????? A)??????? NO₂⁺??

B)??????? NO₂^-

??????????? C)??????? SO₃

??????????? D)??????? SO₄^-2

???????????????????????

25.?????? Which of the following elements is assigned the highest electronegativity value?

??????????? A)??????? K

??????????? B)??????? Ba

??????????? C)??????? Si

??????????? D)??????? Br

??????????? E)??????? As

???????????

26.?????? Which of the following is/are ?an exception to the octet rule?

??????????? A)??????? SO₃^2?

??????????? B)??????? CF₄

??????????? C)??????? NH₃

??????????? D)??????? CO₂

??????????? E)??????? BF₃

??????????? F)??????? NO

???????????

27.?????? The Lewis structure of

??????????? A)??????? PH₃ has ________ bonding pairs and _______lone pairs.

??????????? B)??????? CO₃^-2 ________ bonding pairs and _______lone pairs.

??????????? C)??????? ClO₃^- has ________ bonding pairs and _______lone pairs.

???????????

28.?????? Draw the Lewis dot structure and predict the geometry, hybridization? for the following

??????????? A)??????? ? XeF₄ ?

??????????? B)??????? ? SO₂

??????????? C)??????? CF₄

??????????? D)??????? SF₄

E) ?????? SO₃^-2

F) ?????? SO₂

G) ?????? NO₂^-

???????????????????????

29.?????? Label the ?following compounds as polar, nonpolar or ionic?

??????????? A)??????? XeF₂

??????????? B)??????? HCl

??????????? C)??????? SO₂

??????????? D)??????? H₂S

??????????? E)??????? Na₂O

???????????

30.?????? What are the hybrid orbitals of central atom involved in the bonding in?

??????????? A)??????? sulfur dioxide

??????????? B)??????? sulfur tri oxide ???????????

C)??????? Carbon dioxide

31.?????? List all strong acids and bases

32.?????? Label the following as soluble or ?insoluble in water?

??????????? A)??????? (NH₄)₂CO₃

??????????? B)??????? AgBr

??????????? C)??????? CuSO₄

??????????? D)??????? AlI₃

??????????? E)??????? KNO₃

33.?????? What is the oxidation number of underlined element in each of the following, is

??????????? A)??????? KCrO₂???????????

B)??????? Na ₂Cr ₂O₇

??????????? C)??????? Al₂(SO₄)₃

??????????? ?

???????????

34.?????? Calculate the molarity of the final solution that contains

??????????? A)??????? 45.0 g of KOH in 560.0 mL of solution.

??????????? B)??????? 34 g of Na₂SO₄ in 750.0 mL of solution.

??????????? C) 20 ml of 1.5 molar HCl that is diluted to 175 ml.

???????????

35.?????? How many sigma and pi bonds are in the following molecule?

????????????????????????????????????????????????????????????? ?????

???????????

36.?????? Calculate the ?moles in a gas sample occupying 0.75 L at 180 mmHg and 65?C?

???????????

37.?????? Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of

85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average

atomic mass of rubidium?

38. Titanium has five common isotopes: 46Ti (8.0%), 47Ti (7.8%), 48Ti (73.4%),

49Ti (5.5%), 50Ti (5.3%). What is the average atomic mass of titanium?

39. Calculate the

Number of Oxygen atoms in 34.56 g of Al₂O_3.

Number of molecules of SO₂ in 34.23 g of SO₂

Mass of 3.4 10²² molecules of PH₃

What?s the empirical formula of a molecule containing 18.7% lithium, 16.3% carbon, and 65.0% oxygen?

SO₃

SCl₂

SO₄^-2

• _??Calculate the volume occupied by 56.2 g of SO₂ at 0.87 atm and 45?C. R = 0.08206 L?atm/K?mol.

??for 6 CO2(g)? +? 6 H2O(l)? ?? C6H12O6(s)? +? 6 O2(g)?

_. The combination of coke and steam produces a mixture called coal gas, which can be used as a fuel or as a starting material for other reactions.? If we assume coke can be represented by graphite, the equation for the production of coal gas is

??????????? ?

Calculate the mass of glucose formed by the reaction of 34.5 g of CO2(g)? with 65.2 g? H2O according to following balanced equation.?

6 CO2(g)? +? 6 H2O(l)? ?? C6H12O6(s)? +? 6 O2(g)

A rectangle object is 6.8 cm by 1.2 inch.? What is the area in unit of cm²_?

Define oxidation and reduction.

Name the laws that trell the raltionship between

pressure and volume

Volume and temperature

?Moles and volume.

Partial pressure and total pressure

20 g of metal at 150 ^oC colles to 25⁰C. what si the amount of heat that is lost. Specific heat of metal is 1.2 J/g^oC.

Calculate the wavelength that is associated with 1.2 x10-20 J/quantum?

What is the relationship between energy, wavelength and frequency? Write all statements that are valid.

Solids have _______packed molecules and therefore? tend to have high________point.

Which one of the following group of the elements? is most electronegative?

S, Oxygen, Chlorine, Barium, Potassium, Florine.

A _____ value of? ?H? means the reaction is _______and a negative value indicates it is? _______.

What subshell has the quantum numbers

?n = 4, l = 3, m₁ = ?1

n = 3, l = 0, m₁ = 0

??n = 5, l = 2, m₁ = ?1

A 123 g sample of metal at 67.0?C is added to 200.0 g of H₂O at 15.0?C. The temperature rises to 32.8?C. Assuming that the calorimeter is a perfect insulator, what is the specific heat of the metal? Look up specific heat of H₂O.

For the balanced equation shown below, if the reaction of 0.112 grams of H₂ with excess Fe3O4 0.745 grams of H₂O was the actual yield of the water, what is the percent yield?

Fe3O4+4H2=>3Fe+4H2O

Calculate moles of gas in a sample occupying 0.340 L at 455 mmHg and 56?C?

Calculate the average atomic weight for each of the following elements given the information about isotopes. ?

Magnesium

mass number	exact weight	percent abundance
24	23.985042	78.99
25	24.985837	10.00
26	25.982593	11.01

Molybdenum

mass number exact weight percent abundance 92 91.906808 14.84 94 93.905085 9.25 95 94.905840 15.92 96 95.904678 16.68 97 96.906020 9.55 98 97.905406 24.13 100 99.907477 9.63

• Bond angles in trigonal planar, tetrahedral, bent, linear, octahedral and trigonal bipyramidal molecules are respectively.
• A bond in which an electron pair is shared equally by two atoms is? ______ and the one that shares unequally is __________.

For an endothermic process is _________and is ______for an exothermic process.

Pick the element with the smallest and largest radius from the list in each group based on trend in the periodic table.

Barium, Sodium , Aluminum, Silicon, Sulfur

Chlorine, potassium, gallium, fluorine

Pick the element with the smallest and largest ionization energy from the list in each group based on trend in the periodic table.

Calcium, potassium, arsenic, bromine, gallium

Phosphorous, sulfur, silicon, chlorine

Write possible ions of sulfur, aluminum, chlorine, calcium and potassium that are isoelectronic with argon.

Final exam review Chem 1411 Spring 2015 This is only a review. You are responsible for all
material covered in the course.
Prepared by
Prof. Alka Shukla
Department of Natural Science
HCCS Northeast
1.

Do the following calculations and write the best answer?
A) (12.345 + 0.450 + 45.4)
B) (12.134 + 0.510 ) / 29.4
C) 34.175 x (0.990 + 78.4)

2.

A) What is the mass of a 123.4 mL sample if density is 1.74 g/mL?
B) What is the volume of a 450 Kg sample if density is 0.94 g/mL?

3.
Write the strongest intermolecular interactions for each of the following molecules and predict which
one is likely to have highest boiling point.
A)
CH3CH2 CH2OH
B)
C)
D)
E)
4.

CH3CH2O CH2CH3
CH3CH2 NH2
CH3CH2 CH2CH3
CH3CH2 CH2Cl

List the following is an example of a chemical change or physical change?
A)
water boiling
B)
Snow melting
C)
Hydrogen gas tank exploding
D)
Lake water evaporating during summer
E)
solid carbon di oxide vaporizing
F)
Candle burning

5.
Write the symbols the elements silver, Antimony, tin, chlorine, Sodium, phosphorus, potassium, arsenic
and sulfur .
6.
ion.

Write the formula of Sulfate ion, phosphate ion, Chlorate ion, Bi sulfite ion, hydroxide ion, the nitrate

7.

Write the formulae / names and molar mass of the following compounds
A)
Potassium carbonate

B)
Barium sulfate
C)
Ammonium sulfate
D)
Copper( I) phosphate
E)
Chromium( IV) sulfide
F) FeCl2
G) a compound formed between magnesium and nitrate ions.
H) a compound formed between potassium and sulfide ions.
I) NH4NO3
8.

Calculate the number of moles in
A) 23.45 g of Iron
B) 56.45 g of Arsenic

9.
Write the empirical formula of
A) C2H6
B) C3H8
10.

Balance the following equations and sum the coefficients
A)

____ Na3PO4 + ____ KOH --->. ____ NaOH + ____ K3PO4

B)

____ SO2 + ____ Li2Se --->. ____ SSe2 + ____ Li2O

E)

__ N2H4 + __ N2O4---->. __ N2 + __ H2O

11. At 50?C and 0.5 atm pressure, it is found that 3.24 L of gas weighs 1.11 g molar mass
is:
12. Determine the empirical formula of a compound that is composed of 36.5% sodium, 25.4% sulfur, and
38.1% oxygen and molar mass was 378 g/mole
13.
Calculate the moles of CO2 produced when 3 moles of C3H8(g) reacts with 13 moles of O2.
C3H8(g) + 5O2(g) 3 CO2(g) + 4H2O(1)

14.

A 123.0-g sample of metal at 67.0?C is added to 150.0 g of H2O at 25.0?C. The temperature rises to
24.3?C. Assuming that the calorimeter is a perfect insulator, what is the specific heat of the metal?
(Specific heat of H2O is 4.18 J/g ? ?C.)

15.

Using the H?f following data, determine the heat of reaction for the combustion of
A) C2H4(g) + 3O2(g)-- 2CO2(g) + 2H2O(1)
B) C3H8(g) + 5O2(g) -- 3 CO2(g) + 4H2O(1)

16.

According to the quantum theory, what is the energy contained in a single quantum with
2

a frequency of 5.67 ? 1014 s?1?
17.

Which the name and symbol of quantum number describes the?
A)
orientation in space of an orbital
B)
Spin of electron

18. Perform the following conversions
A)
B)
C)
D)
E)
19.

56oF to kelvin scale
145 K to oF
23.6 miles to cm
5 ft 6 inches to cm
145 Lb to kg
The maximum number of electrons that can occupy the
A)
5f orbitals
B)
4d orbitals
C)
7 s orbitals
D)
3p orbitals
E) 4th shell
F) 3rd shell
G) A single 3d orbital

20.

Which one of the following species will have chemical properties most similar to those of
The Nitrogen atoms
A)
Oxygen atom
B)
fluorine atom
C)
nitride ion
D)
sulfide ion
E)
phosphorous atoms

21.

The elements having the electron configurations
A)
ns2 np5 are called
B)
ns2 called
C)
ns2 np6 are called

22. Arrange in terms of largest to smallest radius.
A)
K, Al, S, As, Br
B)
C, Cl, N, S, Na
23.

What is the electron configuration of
A) Fe+3
B) Sn+2

24.

What is the total number of valence electrons in the
A)
NO2+
B)
NO2C)
SO3
D)
SO4-2
3

25.

Which of the following elements is assigned the highest electronegativity value?
A)
K
B)
Ba
C)
Si
D)
Br
E)
As

26.

Which of the following is/are an exception to the octet rule?
A)
SO32?
B)
CF4
C)
NH3
D)
CO2
E)
BF3
F)
NO

27.

The Lewis structure of
A)
PH3 has ________ bonding pairs and _______lone pairs.
B)
CO3-2 ________ bonding pairs and _______lone pairs.
C)
ClO3 - has ________ bonding pairs and _______lone pairs.

28.

Draw the Lewis dot structure and predict the geometry, hybridization for the following
A)
XeF4
B)
SO2
C)
CF4
D)
SF4
E)
SO3-2
F)
SO2
G)
NO2-

29.

Label the following compounds as polar, nonpolar or ionic?
A)
XeF2
B)
HCl
C)
SO2
D)
H2S
E)
Na2O

30.

What are the hybrid orbitals of central atom involved in the bonding in?
A)
sulfur dioxide
B)
sulfur tri oxide
C)
Carbon dioxide

31.

List all strong acids and bases

32.

Label the following as soluble or insoluble in water?
A)
(NH4)2CO3
B)
AgBr
C)
CuSO4
D)
AlI3
4

E)

KNO3

33.

What is the oxidation number of underlined element in each of the following, is
A)
KCrO2
B)
Na 2Cr 2O7
C)
Al2(SO4)3

34.

Calculate the molarity of the final solution that contains
A)
45.0 g of KOH in 560.0 mL of solution.
B)
34 g of Na2SO4 in 750.0 mL of solution.
C) 20 ml of 1.5 molar HCl that is diluted to 175 ml.

35.

How many sigma and pi bonds are in the following molecule?
H3 C - CH = CH - C
N:

36.

Calculate the moles in a gas sample occupying 0.75 L at 180 mmHg and 65?C?

37.
Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of
85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average
atomic mass of rubidium?
38. Titanium has five common isotopes: 46Ti (8.0%), 47Ti (7.8%), 48Ti (73.4%),
49Ti (5.5%), 50Ti (5.3%). What is the average atomic mass of titanium?
39. Calculate the
A) Number of Oxygen atoms in 34.56 g of Al2O3.
B) Number of molecules of SO2 in 34.23 g of SO2
C) Mass of 3.4 1022 molecules of PH3
40.

What?s the empirical formula of a molecule containing 65.5% carbon, 5.5%
hydrogen, and 29.0% oxygen? If the molar mass of the compound is 110
grams/mole, what?s the molecular formula?

41.

What?s the empirical formula of a molecule containing 18.7% lithium, 16.3% carbon,
and 65.0% oxygen?

42.

Draw the lewis structure and give the hybridization and geometry of

A) SO3
B) SCl2
C) SO4-2
Calculate the volume occupied by 56.2 g of SO2 at 0.87 atm and 45?C. R = 0.08206 Latm/Kmol.
o
44. Calculate Hrxn for 6 CO2(g) + 6 H2O(l) C6H12O6(s) + 6 O2(g)
43.

5

45.

From the following heats of reaction

2 SO2(g) + O2(g) 2 SO3(g)H = ? 196 kJ
2 S(s) + 3 O2(g) 2 SO3 (g)H = ? 790 kJ
Calculate the heat of reaction for

S(s) + O2(g) SO2(g) H = ? kJ
46.

The combination of coke and steam produces a mixture called coal gas, which can be used as a
fuel or as a starting material for other reactions. If we assume coke can be represented by graphite,
the equation for the production of coal gas is
.

2 C (s) 2 H2O (g)

CH4 (g) CO2(g)

Determine the standard enthalpy change for this reaction from the following
standard enthalpies of reaction :
(1) C(s) H2O (g) CO (g) H2 (g)
(2) CO (g) H2O (g) CO2 (g) H2 (g)

H 131.3 kJ
H - 41.2 kJ

(3) CH4 (g) H2O (g)

H 206.1 kJ

47.

3 H2 (g) CO (g)

Calculate the mass of glucose formed by the reaction of 34.5 g of CO 2(g) with 65.2 g
H2O according to following balanced equation.

6 CO2(g) + 6 H2O(l) C6H12O6(s) + 6 O2(g)
48.
49.
50.

51.
52.
53.
54.
55.
56.
57.

A rectangle object is 6.8 cm by 1.2 inch. What is the area in unit of cm2 ?
Define oxidation and reduction.
Name the laws that trell the raltionship between
a. pressure and volume
b. Volume and temperature
c. Moles and volume.
d. Partial pressure and total pressure
20 g of metal at 150 oC colles to 250C. what si the amount of heat that is lost. Specific heat
of metal is 1.2 J/goC.
Calculate the wavelength that is associated with 1.2 x10-20 J/quantum?
What is the relationship between energy, wavelength and frequency? Write all statements
that are valid.
Solids have _______packed molecules and therefore tend to have high________point.
Which one of the following group of the elements is most electronegative?
S, Oxygen, Chlorine, Barium, Potassium, Florine.
A _____ value of ?H means the reaction is _______and a negative value indicates it is
_______.
What subshell has the quantum numbers
a. n = 4, l = 3, m1 = ?1
b. n = 3, l = 0, m1 = 0
c. n = 5, l = 2, m1 = ?1
6

A 123 g sample of metal at 67.0?C is added to 200.0 g of H 2O at 15.0?C. The temperature
rises to 32.8?C. Assuming that the calorimeter is a perfect insulator, what is the specific
heat of the metal? Look up specific heat of H 2O.
59. For the balanced equation shown below, if the reaction of 0.112 grams of H 2 with excess
Fe3O4 0.745 grams of H2O was the actual yield of the water, what is the percent yield?
58.

60.
61.

Fe3O4+4H2=>3Fe+4H2O
Calculate moles of gas in a sample occupying 0.340 L at 455 mmHg and 56?C?
Calculate the average atomic weight for each of the following elements given the
information about isotopes.

a. Magnesium
mass number

exact weight

percent abundance

24

23.985042

78.99

25

24.985837

10.00

26

25.982593

11.01

b.
c. Molybdenum
mass number exact weight percent abundance
92
91.906808
14.84
94
93.905085
9.25
95
94.905840
15.92
96
95.904678
16.68
97
96.906020
9.55
98
97.905406
24.13
100
99.907477
9.63

Bond angles in trigonal planar, tetrahedral, bent, linear, octahedral and trigonal bipyramidal
molecules are respectively.
63. A bond in which an electron pair is shared equally by two atoms is ______ and the one that shares
unequally is __________.
62.

64.
65.

For an endothermic process is _________and is ______for an exothermic process.
Pick the element with the smallest and largest radius from the list in each group based on
trend in the periodic table.
a. Barium, Sodium , Aluminum, Silicon, Sulfur
b. Chlorine, potassium, gallium, fluorine

Pick the element with the smallest and largest ionization energy from the list in each group
based on trend in the periodic table.
a. Calcium, potassium, arsenic, bromine, gallium
b. Phosphorous, sulfur, silicon, chlorine
66.

7

67.

Write possible ions of sulfur, aluminum, chlorine, calcium and potassium that are
isoelectronic with argon.

8

9