wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Honors Chem Final Exam Reivew

Total questions: 78

Worksheet time: 3hrs 18mins

Name
Class
Date
1.

The atomic mass for this element is __________.

a)

26

b)

Fe

c)

55.845

d)

iron

2.

How many electrons can the d sublevel hold?

a)
8
b)
10
c)
2
d)
4
3.

How many electrons can the p sublevel hold?

a)
8
b)

6

c)
2
d)
4
4.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

5.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
6.

Which orbital is displayed correctly?

a)

A

b)

B

c)

C

d)

D

7.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
8.

What atom matches this electron configuration?

[Xe] 6s25d8

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

9.

Rank the energy of the sublevels from lowest to highest (lowest energy on left)

a)

s

b)

p

c)

d

d)

f

1)
2)
3)
4)
10.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
11.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
12.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
13.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
14.

Elements that are poor conductors, dull, and have a low melting point

a)

metals

b)

non-metals

c)

metalloids

15.

Positive ions are called

a)

anions

b)

cations

16.

When an atom gains an electron, the size of atom

a)

will increase

b)

will decrease

c)

will not change

17.

When an atom loses an electron the size of atom

a)

will increase

b)

will decrease

c)

will not change

18.

Anions have ionic radii that are larger than their atomic radii.

a)

True

b)

False

19.

Which species has the larger radius?

a)

Cl

b)

Cl-

20.

Place the chlorine, aluminum, phosphorus and magnesium in order of decreasing atomic radius.

a)

chlorine, aluminum, phosphorus, magnesium

b)

aluminum, phosphorus,magnesium, chlorine

c)

aluminum, phosphorus, chlorine, magnesium

d)

Magnesium, aluminum, phosphorus, chlorine

21.

How many valence electrons does Carbon have?

a)

4

b)

6

c)

12

d)

14

22.

What is the atomic number of iron?

a)

30

b)

24

c)

26

d)

28

23.

What is the symbol for the element with atomic number 11?

a)

K

b)

Cs

c)

Na

d)

Rb

24.

What is the atomic mass of lithium?

a)

85.47

b)

39.10

c)

22.99

d)

6.94

25.

Changing the number of ELECTRONS ____ the identity of the atom.

a)

changes

b)

does NOT change

26.
What is the name of the pictured isotope?
a)
Copper-29
b)
Copper-63
c)
Copper-34
d)
CopperWopperHopperBopper
27.

How many neutrons are in the isotope pictured above?

a)

29

b)

34

c)

63

d)

92

28.

How many neutrons are in Sodium-20?

a)

9

b)

11

c)

20

d)

0

29.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
30.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
31.

Ionic or Covalent?

As2O5 (Hint: As is a metalloid that can act as a nonmetal)

a)

Ionic

b)

Covalent

32.

Why are ionic compounds typically more brittle than covalent compounds?

a)

The molecular bonds in ionic compounds are very flexible.

b)

The ionic bonds form a rigid lattice that can shatter when stressed.

c)

Covalent bonds are much weaker than ionic bonds.

d)

Ionic compounds are not more brittle; it is the other way around.

33.

Which of the following is a characteristic feature of substances with covalent bonds?

a)

High solubility in water.

b)

High electrical conductivity in solid form.

c)

Low boiling points.

d)

High melting points.

34.

What type of bond will conduct electricity in a dissolved state?

a)

ionic

b)

covalent

35.
What is the formula for calcium chloride
a)
CaCl
b)
CaCl2
c)
Ca2Cl
d)
CaCl3
36.
Barium and Selenium form ?
a)
BaSe
b)
Ba2Se
c)
Ba2Se2
d)
BaSe2
37.

What is the formula for Sodium  Sulfide? 

a)

Na2S

b)

NaS2

c)

Na2S2

d)

NaS

38.

Where are the transition metals located on the periodic table?

a)

blue square

b)

red square

c)

yellow square

39.

What is the correct name for this compound?

a)

fluorine chlorine

b)

iron chloride

c)

iron(II) chloride

d)

iron(I) chloride

40.

What is the formula for iron(III) oxide?

a)

FeO

b)

Fe(III) O

c)

Fe2O3

d)

Fe3O2

41.

3Ca + 2AlCl3 → 3CaCl2 + 2Al

a)

Synthesis

b)

Single Displacement

c)

Double Displacement

d)

Decomposition

42.

Determine the reaction type: 4Si + S8 → 4SiS2

a)

Double displacement

b)

Single Displacement

c)

Synthesis

d)

Decomposition

43.

Balance the equation: __P4 + __O2 → __P2O3

a)

balanced

b)

1, 2, 3

c)

2, 1, 3

d)

1, 3, 2

44.
What are the products of this reaction?
Cu+ AgNO3--> 
a)
Cu(NO3)2+Ag
b)
CuNO3 + Ag
c)
CuAg+NO3
d)
Cu+ AgNO3
45.
in a reaction, aqueous barium chloride reacts with aqueous potassium carbonate to produce solid barium carbonate and aqueous potassium chloride. what is the correct balanced equation.
a)
Ba2Cl(aq) + KCO3(aq) --> BaCO3(s) + KCl(aq)
b)
BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + 2KCl(aq)
c)
BaCl(aq) + K2CO3(aq) --> BaCO3(s) + K2Cl(aq)
d)
Ba2Cl2(aq) + KCO3(aq) --> Ba2CO3(s) + KCl2(aq)
46.

What are the products of this single replacement reaction: Mg + CuSO4

a)

Cu + MgSO4

b)

Cu + SO4Mg

c)

Cu + Mg(SO4)2

d)

No Reaction

47.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

48.

How many significant figures are in the number 2.53 x 10^5?

a)

2

b)

3

c)

4

d)

5

e)

6

49.

Which of the following has four significant figures?

a)

10001

b)

1000

c)

0.01204

d)

0.010

50.

Solve the following with the correct decimal places:

14.10 + 12.10 + 10.112

51.
Change from standard form to scientific notation: 0.004078
a)
4.078  x  10-3
b)
4.078  x  103
c)
40.78  x  10-4
d)
.4078  x  10-2
52.
You know 1000 mg = 1 g.  Convert 2.5 grams into milligrams.
a)
25 mg
b)
25,000 mg
c)
250 mg
d)
2500 mg
53.
32.9 km = ___________ cm
a)
32,900
b)
329,000
c)
3,290,000
d)
32,900,000
54.

Which element is formed from plutonium-240 during alpha decay?

a)

Uranium-236

b)

Thorium-232

c)

Lead-206

d)

Radon-222

55.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
56.
Has the highest penetrating power.  Can penetrate our body.  Even several cm thick of lead or several meters thick of concrete cannot stop all of it.
a)
Alpha
b)
Beta
c)
Gamma
57.
If we start off with element 24X50 after an alpha decay we get another element Y that looks like
a)
22Y50
b)
22Y46
c)
20Y48
d)
26Y54
58.
Determine the mass of
1.4 x 1023 atoms of Chromium.
a)
7.3 x 1024 g
b)
0.23 g
c)
4.4 x 1048g
d)
12 g
59.
2NaClO3 (s) → 2NaCl (s) + 3O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
60.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
61.
N2 +  3H2 −->  2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
62.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
63.

Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 

a)

Mg

b)

H2

c)

MgCl2

d)

HCl

64.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
65.

What is the volume of 1.75 mol CO2?

a)

39.2 L

b)

0.078 L

c)

11.2 L

d)

22.4 L

66.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
67.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
68.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
69.

What is the significance of boiling point in determining intermolecular forces?

a)

The boiling point has no relation to intermolecular forces.

b)

Higher boiling points suggest weaker intermolecular forces.

c)

The boiling point indicates the molecular weight of a substance.

d)

Higher boiling points suggest stronger intermolecular forces.

70.

How do dipole-dipole interactions occur?

a)

Dipole-dipole interactions occur between nonpolar molecules, where the positive end of one molecule is repelled by the negative end of another.

b)

Dipole-dipole interactions occur between polar molecules, where the positive end of one molecule is attracted to the negative end of another.

c)

Dipole-dipole interactions occur between ionic compounds, where the positive ions attract the negative ions.

d)

Dipole-dipole interactions occur between gases, where the molecules collide and interact randomly.

71.

What type of intermolecular forces does NH3 exhibit?

a)

Only hydrogen bonding

b)

Hydrogen bonding, dipole-dipole interactions, and London dispersion forces

c)

Only dipole-dipole interactions

d)

Only London dispersion forces

72.

Which molecule has the weakest intermolecular forces: HCl, NH3, or Br2?

a)

HCl

b)

NH3

c)

Br2

d)

CH4

73.

What is the strongest type of intermolecular force?

a)

Dipole-dipole interactions

b)

London dispersion forces

c)

Hydrogen bonding

d)

Ionic bonding

74.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)
CBr4
d)
PCl3
75.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
76.

When you have Zn-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

77.

NaNO3 soluble (aq) or insoluble (s)?

a)

Soluble (aq)

b)

Insoluble (s)

78.
Calculate the Formal Charge for the Oxygen Labeled 1 
a)
-1
b)
+1
c)
0
d)
-2

Similar Resources on Wayground

Subatomic Particles Practice MR

76 questions

Subatomic Particles Practice MR

quiz

Worksheet

•

9th - 12th Grade

HC05 Binary Covalent Nomenclature

74 questions

HC05 Binary Covalent Nomenclature

quiz

Worksheet

•

10th - 11th Grade

ÔN TẬP HÓA 10 BÀI 17, 18

79 questions

ÔN TẬP HÓA 10 BÀI 17, 18

quiz

Worksheet

•

9th - 12th Grade

Chemistry Basics Review

80 questions

Chemistry Basics Review

quiz

Worksheet

•

9th - 12th Grade

ÔN TẬP GIỮA KÌ I HÓA 11

82 questions

ÔN TẬP GIỮA KÌ I HÓA 11

quiz

Worksheet

•

10th Grade

AQA GCSE Chemistry Paper 1

74 questions

AQA GCSE Chemistry Paper 1

quiz

Worksheet

•

10th - 11th Grade

Ôn tập học kì 2 lớp 10 2021 2022

73 questions

Ôn tập học kì 2 lớp 10 2021 2022

quiz

Worksheet

•

10th Grade

Periodic table groups

75 questions

Periodic table groups

quiz

Worksheet

•

10th - 12th Grade