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Chemistry Final Study Guide — Worksheet Questions (Grade 10)

Total questions: 114

Worksheet time: 57mins

Name
Class
Date
1.

Use the pictures showing a robot causing water displacement in a graduated cylinder and a digital scale reading to determine the robot’s volume. Report the volume with proper units.

a)

1.2 mL1.2\ \text{mL}

b)

1.6 mL1.6\ \text{mL}

c)

2.0 mL2.0\ \text{mL}

d)

0.8 mL0.8\ \text{mL}

2.

According to the scale shown, what is the mass of the robot? Use proper units.

a)

3.20 g3.20\ \text{g}

b)

4.32 g4.32\ \text{g}

c)

5.00 g5.00\ \text{g}

d)

4.23 g4.23\ \text{g}

3.

Using the measured mass and volume, what is the density of the robot? Use proper units.

a)

2.7 g/mL2.7\ \text{g/mL}

b)

3.0 g/mL3.0\ \text{g/mL}

c)

4.5 g/mL4.5\ \text{g/mL}

d)

1.6 g/mL1.6\ \text{g/mL}

4.

Based on the calculated density and the table of densities for titanium (4.5 g/mL), iron (7.8 g/mL), gold (19.3 g/mL), silver (10.5 g/mL), and aluminum (2.7 g/mL), what metal is the robot made of?

a)

Titanium

b)

Iron

c)

Aluminum

d)

Silver

5.

What lab equipment was used to measure the volume of the robot?

a)

Graduated cylinder

b)

Beaker

c)

Volumetric flask

d)

Burette

6.

What lab equipment was used to measure the mass of the robot?

a)

Digital balance

b)

Triple-beam lever

c)

Volumetric flask

d)

Pipette

7.

Locate phosphorus (P, #15) on the periodic table. How many protons does a neutral phosphorus atom have?

a)

14

b)

15

c)

16

d)

32

8.

Locate phosphorus (P, #15) on the periodic table. How many total electrons does a neutral phosphorus atom have?

a)

14

b)

15

c)

16

d)

31

9.

For the common phosphorus isotope with mass number 31, how many neutrons does the atom have?

a)

14

b)

15

c)

16

d)

31

10.

How many valence electrons does a neutral phosphorus atom have?

a)

3

b)

4

c)

5

d)

6

11.

How many electron shells (energy levels) does a neutral phosphorus atom have?

a)

2

b)

3

c)

4

d)

5

12.

What would happen to phosphorus if you added one proton?

a)

It would become silicon.

b)

It would become sulfur.

c)

It would become an isotope of phosphorus.

d)

It would become chlorine.

13.

What would happen to phosphorus if you added a neutron? What is it called when you change the number of neutrons in an atom?

a)

It becomes an ion; the change is called ionization.

b)

It becomes a different element; the change is called transmutation.

c)

It remains phosphorus; the change is called forming an isotope.

d)

It remains phosphorus; the change is called electronegativity.

14.

Write the isotope symbol for Phosphorus-32 and determine its number of neutrons.

a)

1532P^{32}_{15}\text{P} ; 16 neutrons

b)

1532P^{32}_{15}\text{P} ; 17 neutrons

c)

1632S^{32}_{16}\text{S} ; 16 neutrons

d)

1531P^{31}_{15}\text{P} ; 16 neutrons

15.

Identify all missing items in the nuclear equation and the reaction type: ____ → 93239Np^{239}_{93}\text{Np} + 24He^{4}_{2}\text{He} . What kind of reaction is this?

a)

95243Am^{243}_{95}\text{Am} ; alpha decay

b)

94239Pu^{239}_{94}\text{Pu} ; beta decay

c)

92235U^{235}_{92}\text{U} ; fission

d)

95243Am^{243}_{95}\text{Am} ; gamma emission

16.

Barium-140 undergoes beta decay. Write the complete nuclear equation showing this transformation: 56140Ba^{140}_{56}\text{Ba} → ______ + ______.

a)

55140Cs^{140}_{55}\text{Cs} + +10β^{0}_{+1}\beta

b)

57140La^{140}_{57}\text{La} + −10β^{0}_{-1}\beta

c)

54136Xe^{136}_{54}\text{Xe} + 24α^{4}_{2}\alpha

d)

56140Ba^{140}_{56}\text{Ba} + γ\gamma

17.

Hydrogen-1 has what name and how many neutrons?

a)

Protium; 0 neutrons

b)

Deuterium; 1 neutron

c)

Tritium; 2 neutrons

d)

Protium; 1 neutron

18.

Hydrogen-2 has what name and how many neutrons?

a)

Protium; 0 neutrons

b)

Deuterium; 1 neutron

c)

Tritium; 2 neutrons

d)

Deuterium; 2 neutrons

19.

Hydrogen-3 has what name and how many neutrons?

a)

Protium; 0 neutrons

b)

Deuterium; 1 neutron

c)

Tritium; 2 neutrons

d)

Tritium; 3 neutrons

20.

Across a period in the periodic table, how does atomic radius change?

a)

It increases.

b)

It decreases.

c)

It stays the same.

d)

It fluctuates randomly.

21.

Down a group in the periodic table, how does atomic radius change?

a)

It increases.

b)

It decreases.

c)

It stays the same.

d)

It alternates increase/decrease each period.

22.

Across a period, how does electronegativity generally change?

a)

It increases.

b)

It decreases.

c)

It remains constant.

d)

It drops sharply then rises.

23.

Down a group, how does electronegativity generally change?

a)

It increases.

b)

It decreases.

c)

It remains constant.

d)

It oscillates without a trend.

24.

Across a period, how do valence electrons change?

a)

They decrease from left to right.

b)

They increase from left to right.

c)

They remain the same.

d)

They reset every two elements.

25.

Down a group, how do valence electrons change?

a)

They increase.

b)

They decrease.

c)

They remain the same for elements in the group.

d)

They double each period.

26.

Across a period, how does ionization energy generally change?

a)

It increases.

b)

It decreases.

c)

It is constant.

d)

It has no pattern.

27.

Down a group, how does ionization energy generally change?

a)

It increases.

b)

It decreases.

c)

It is constant.

d)

It spikes for noble gases only.

28.

Across a period, how does atomic mass generally change?

a)

It increases.

b)

It decreases.

c)

It remains constant.

d)

It alternates increase/decrease.

29.

Down a group, how does atomic mass generally change?

a)

It increases.

b)

It decreases.

c)

It remains constant.

d)

It shows no trend.

30.

Which element is expected to have the smaller atomic radius—Al or In?

a)

Aluminum (Al)

b)

Indium (In)

c)

Both are the same

d)

Cannot be determined

31.

Which element is expected to have the greater atomic mass—Na or K?

a)

Sodium (Na)

b)

Potassium (K)

c)

Both are the same

d)

Cannot be determined

32.

Which element is expected to be more electronegative—Cs or Na?

a)

Cesium (Cs)

b)

Sodium (Na)

c)

Both are the same

d)

Cannot be determined

33.

Which element is expected to have the lower ionization energy—Ca or Sr?

a)

Calcium (Ca)

b)

Strontium (Sr)

c)

Both are the same

d)

Cannot be determined

34.

Why is the ionization energy of Sr expected to be lower than that of Ca?

a)

Sr has a smaller radius and stronger attraction to its electrons.

b)

Sr has a larger radius and more shielding, so outer electrons are easier to remove.

c)

Sr has fewer electrons in total, so its energy is lower.

d)

Sr is more electronegative, so it loses electrons readily.

35.

Which two elements have similar properties to Mg (magnesium)?

a)

Be and Ca

b)

Na and K

c)

C and Si

d)

Al and Ga

36.

For bond types, which statement correctly describes ionic bonding versus covalent bonding?

a)

Ionic: formed between metals and nonmetals; electrons are transferred. Covalent: formed between nonmetals; electrons are shared.

b)

Ionic: formed between nonmetals; electrons are shared. Covalent: formed between metals; electrons are transferred.

c)

Ionic: formed between noble gases; electrons are donated. Covalent: formed between halogens; electrons are received.

d)

Ionic: formed between metalloids only; electrons are delocalized. Covalent: formed between metals only; electrons are donated.

37.

The bond between sodium and fluorine is ________.

a)

Ionic

b)

Covalent

c)

Metallic

d)

Hydrogen

38.

The bond between carbon and hydrogen is ________.

a)

Ionic

b)

Covalent

c)

Metallic

d)

Hydrogen

39.

What is the formula for the compound that results when magnesium bonds with arsenic?

a)

MgAs

b)

MgAs2

c)

Mg3As2

d)

Mg2As3

40.

What is the formula for the compound that results when sodium bonds with the sulfate ion (SO4)2−(\text{SO}_4)^{2-} ?

a)

NaSO4

b)

Na2SO4

c)

NaSO3

d)

Na2SO3

41.

How many bonds does Arsenic need to make to fill its valence shell?

a)

1 bond

b)

2 bonds

c)

3 bonds

d)

4 bonds

42.

How many bonds does Sulfur need to make to fill its valence shell?

a)

1 bond

b)

2 bonds

c)

3 bonds

d)

4 bonds

43.

Scientific Method: A group of students is conducting the following experiment. Lab 12: What’s Up With Mass? Purpose: To determine the effect of the mass of a cart upon its acceleration when the forces acting upon it are held constant. What is the independent variable for the experiment above?

a)

mass of the cart

b)

acceleration of the cart

c)

constant force applied

d)

type of surface

44.

Scientific Method: A group of students is conducting the following experiment. Lab 12: What’s Up With Mass? Purpose: To determine the effect of the mass of a cart upon its acceleration when the forces acting upon it are held constant. What is the dependent variable for the experiment above?

a)

acceleration of the cart

b)

mass of the cart

c)

constant force applied

d)

length of the cart

45.

Anna Lytical and Nellie Newton conduct several trials in which they study the effect of varying the mass of a cart upon the acceleration of the cart when pulled with a constant force. Which notebook entry accurately identifies the variables and displays the best choice for a plot?

a)

Notebook Entry A

b)

Notebook Entry B

46.

Significant Figures: Identify the correct amount of significant figures in −0.00567 °C.

a)

2

b)

3

c)

4

d)

5

47.

Significant Figures: Identify the correct amount of significant figures in $198,200.

a)

3

b)

4

c)

5

d)

6

48.

Significant Figures: Identify the correct amount of significant figures in 56.870 kg.

a)

3

b)

4

c)

5

d)

6

49.

Significant Figures: Identify the correct amount of significant figures in 19.697 cm.

a)

3

b)

4

c)

5

d)

6

50.

Significant Figures: Identify the correct amount of significant figures in 23,900 km.

a)

2

b)

3

c)

4

d)

5

51.

Measurement: Measure the black bar shown on the ruler, using the correct number of significant figures and units.

a)

3.0 cm

b)

3.4 cm

c)

2.8 cm

d)

4.0 cm

52.

Measurement: Read the volume at the meniscus of the graduated cylinder, using the correct number of significant figures and units.

a)

42.0 mL

b)

44.0 mL

c)

45.0 mL

d)

48.0 mL

53.

Graphing: Look at the data table of salmon species and their average weights (lbs). Which type of graph would BEST represent the data?

a)

bar graph

b)

line graph

c)

scatter plot

d)

histogram

54.

The following data is taken from Mr. Gulch’s medical records. A data table lists Year and Mr. Gulch’s Weight (kg) for 2005–2011. Identify the dependent variable in the data table.

a)

Year

b)

Mr. Gulch’s weight (kg)

55.

The following data is taken from Mr. Gulch’s medical records. A data table lists Year and Mr. Gulch’s Weight (kg) for 2005–2011. Identify the independent variable in the data table.

a)

Year

b)

Mr. Gulch’s weight (kg)

56.

What should be included in a CER (Claim–Evidence–Reasoning) response? Select all that apply.

a)

Claim

b)

Evidence

c)

Reasoning

57.

Read the CER written below and answer the question. Question: What is the molar ratio of hydrogen gas to oxygen gas that makes the most amount of water? Conclusion (sentences labeled 1–6): 1 In our lab we tested different amounts of hydrogen and oxygen gas mixtures. 2 We found that the 1:5 ratio made the least amount of “pop” sound and the 2:4 ratio made the greatest amount of “pop” sound. 3 When hydrogen and oxygen react they come together in a certain ratio of molecules to make water. 4 The mole ratio in the balanced equation tells you the amount of hydrogen and oxygen that makes the most amount of product (water). 5 The reason why the 1:5 ratio was not the optimal ratio is because there is not enough hydrogen gas molecules to react with all the oxygen molecules. 6 Only in the 2:4 ratio do you have the correct amount of each molecule to make the most water. Which sentence number(s) include the evidence?

a)

1

b)

2

c)

3

d)

4

58.

Periodic Table Organization: What is the symbol for Chlorine?

a)

Cl

b)

Ch

c)

C

d)

Cl2

59.

Periodic Table Organization: What is the atomic number for Chlorine?

a)

16

b)

17

c)

18

d)

35

60.

Periodic Table Organization: How many protons does Chlorine have?

a)

17

b)

18

c)

35

d)

7

61.

Periodic Table Organization: How many electrons does Chlorine have?

a)

17

b)

18

c)

35

d)

7

62.

Periodic Table Organization: How many electron shells (energy levels) does Chlorine have?

a)

2

b)

3

c)

4

d)

5

63.

Periodic Table Organization: How many valence electrons does Chlorine have?

a)

1

b)

5

c)

7

d)

8

64.

Parts of the Atom: Above are the symbols for two isotopes of Phosphorus (Phosphorus-31 and Phosphorus-33). What is different about each of them?

a)

The number of protons

b)

The number of neutrons

c)

The number of electrons

d)

The chemical symbol

65.

Parts of the Atom: How many protons do each isotope have?

a)

14

b)

15

c)

16

d)

31

66.

Parts of the Atom: How many electrons do each isotope have?

a)

15

b)

16

c)

31

d)

33

67.

Parts of the Atom: How many neutrons do each isotope have?

a)

16 for Phosphorus-31 and 18 for Phosphorus-33

b)

15 for Phosphorus-31 and 17 for Phosphorus-33

c)

31 for Phosphorus-31 and 33 for Phosphorus-33

d)

18 for Phosphorus-31 and 20 for Phosphorus-33

68.

Parts of the Atom: Draw a Bohr model that shows the electrons for Phosphorus.

a)

Shells with 2, 8, and 5 electrons

b)

Shells with 2, 7, and 6 electrons

c)

Shells with 2, 8, and 8 electrons

d)

Shells with 1, 8, and 6 electrons

69.

Parts of the Atom: Draw a Lewis dot symbol for Phosphorus.

a)

3 valence electrons shown

b)

4 valence electrons shown

c)

5 valence electrons shown

d)

6 valence electrons shown

70.

Parts of the Atom: Will Aluminum gain or lose electrons?

a)

Gain electrons

b)

Lose electrons

c)

Neither gain nor lose electrons

d)

Gain electrons then lose electrons

71.

Parts of the Atom: What is the oxidation number for Phosphorus?

a)

−3

b)

+3

c)

+5

d)

−2

72.

Metals, Nonmetals and Metalloids: Find Zirconium (#40) on the periodic table. What type of element is it? Would you expect Zirconium to be a good conductor of heat and electricity?

a)

Metal; yes

b)

Metal; no

c)

Metalloid; yes

d)

Nonmetal; no

73.

Metals, Nonmetals and Metalloids: Find Iridium (#77) on the periodic table. What type of element is it? Would you expect Iridium to be a brittle solid?

a)

Metal; yes

b)

Metal; no

c)

Metalloid; yes

d)

Nonmetal; yes

74.

Metals, Nonmetals and Metalloids: Find Fluorine (#9) on the periodic table. What type of element is it? Is Fluorine a gas, liquid or solid at room temperature?

a)

Nonmetal; gas

b)

Nonmetal; liquid

c)

Metalloid; solid

d)

Metal; gas

75.

Metals, Nonmetals and Metalloids: Find Antimony (#51) on the periodic table. What type of element is it? Would you expect Antimony to be ductile?

a)

Metalloid; yes

b)

Metalloid; no

c)

Metal; yes

d)

Nonmetal; no

76.

Families of the Periodic Table: What family is located in group 2A?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

77.

Families of the Periodic Table: What family has 7 electrons in their outer shell?

a)

Halogens

b)

Noble gases

c)

Alkali metals

d)

Transition metals

78.

Families of the Periodic Table: Which is more reactive, Beryllium (#4) or Calcium (#20)?

a)

Beryllium

b)

Calcium

c)

Both equally reactive

d)

Neither is reactive

79.

Families of the Periodic Table: Which is more reactive, Fluorine (#9) or Iodine (#53)?

a)

Fluorine

b)

Iodine

c)

They have equal reactivity

d)

It depends on which metal they react with

80.

Families of the Periodic Table: What is the oxidation number for the Alkali Metals?

a)

+1

b)

+2

c)

−1

d)

0

81.

Families of the Periodic Table: Which noble gas is the most dense?

a)

Helium

b)

Argon

c)

Xenon

d)

Radon

82.

Families of the Periodic Table: Which transition metal in period 3 is the least dense?

a)

Scandium

b)

Copper

c)

Zinc

d)

There are no transition metals in period 3

83.

Periodic Trends (Atomic Radius and Ionization Energy): Which element on the periodic table has the largest atomic radius? The smallest?

a)

Francium largest and Helium smallest

b)

Cesium largest and Hydrogen smallest

c)

Uranium largest and Neon smallest

d)

Potassium largest and Helium smallest

84.

Which element has the larger atomic radius: Calcium (#20) or Barium (#56)?

a)

Calcium (#20)

b)

Barium (#56)

85.

Which element has the larger atomic radius: Calcium (#20) or Arsenic (#33)?

a)

Calcium (#20)

b)

Arsenic (#33)

86.

Which element has the greater ionization energy: Calcium (#20) or Barium (#56)?

a)

Calcium (#20)

b)

Barium (#56)

87.

Which element has the larger ionization energy: Calcium (#20) or Arsenic (#33)?

a)

Calcium (#20)

b)

Arsenic (#33)

88.

What type of bond is between a metal and a nonmetal?

a)

Ionic bond

b)

Covalent bond

c)

Metallic bond

89.

What type of elements become negative ions?

a)

Metals

b)

Metalloids

c)

Nonmetals

90.

In what type of bond are the electrons freely moving about in a “sea of electrons”?

a)

Metallic bond

b)

Ionic bond

c)

Polar covalent bond

91.

Metals have higher electronegativity values compared to nonmetals.

a)

True

b)

False

92.

What is the difference in electronegativity between Sulfur (S) and Bromine (Br)?

a)

About 0.1

b)

About 0.4

c)

About 0.8

d)

About 1.2

93.

What type of bond is between S and Br based on their electronegativity difference?

a)

Ionic

b)

Polar covalent

c)

Nonpolar covalent

94.

What is the difference in electronegativity between Titanium (Ti) and Oxygen (O)?

a)

About 0.5

b)

About 1.0

c)

About 1.9

d)

About 2.5

95.

What type of bond is between Ti and O based on their electronegativity difference?

a)

Ionic

b)

Polar covalent

c)

Nonpolar covalent

96.

What is the difference in electronegativity between Phosphorus (P) and Chlorine (Cl)?

a)

About 0.2

b)

About 0.6

c)

About 1.0

d)

About 1.6

97.

What type of bond is between P and Cl based on their electronegativity difference?

a)

Ionic

b)

Polar covalent

c)

Nonpolar covalent

98.

How many bonds do elements in group 5A typically form in covalent molecules?

a)

One

b)

Two

c)

Three

d)

Four

99.

How many bonds do elements in group 7A typically form in covalent molecules?

a)

One

b)

Two

c)

Three

d)

Four

100.

Select all molecules that have the molecular formula C2H6O.

a)

Ethanol

b)

Dimethyl ether

c)

Acetic acid

d)

Ethane

101.

In the covalent molecule A3H8Bz, where Adamantium (A) is in group 4A and Bazoolium (Bz) is in group 6A, how many covalent bonds does the central atom A typically form?

a)

Two

b)

Three

c)

Four

d)

Five

102.

In the covalent molecule A3H9M, where Mizium (M) is in group 5A, how many covalent bonds does the atom M typically form?

a)

One

b)

Two

c)

Three

d)

Four

103.

What is the molecular geometry around the central atom in NF3?

a)

Linear

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Tetrahedral

104.

What is the molecular geometry around the central atom in AH4 when A is a group 4A element?

a)

Bent

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Tetrahedral

105.

What is the molecular geometry of H2Bz when Bz is a group 6A element?

a)

Linear

b)

Bent

c)

Trigonal planar

d)

Tetrahedral

106.

Do metals gain or lose electrons when forming ions?

a)

Gain electrons

b)

Lose electrons

107.

After becoming ions, what charge do nonmetals typically have?

a)

Positive charge

b)

Negative charge

108.

Bolonium (Bo) is a metal in group 2A and Wonderflonium (Wo) is a nonmetal in group 7A. What is the correct empirical formula for the ionic compound they form?

a)

BoWo

b)

Bo2Wo

c)

BoWo2

d)

Bo2Wo2

109.

Elephantium (E) is a nonmetal in group 5A. What is the formula for Bolonium Elephantide?

a)

BoE

b)

Bo2E3

c)

Bo3E2

d)

BoE3

110.

What is the formula for Bolonium (Bo) nitrate ( NO31−NO_3^{1-} )?

a)

BoNO3

b)

Bo(NO3)2

c)

Bo2(NO3)3

d)

Bo(NO3)3

111.

An unknown substance dissolves in water and melts at a low temperature. What is the bonding type for this substance?

a)

Ionic

b)

Polar covalent (molecular)

c)

Metallic

d)

Network covalent

112.

An unknown substance doesn't conduct electricity when solid but does dissolve in water and will conduct electricity when dissolved. What is the bonding type for this substance?

a)

Ionic

b)

Nonpolar covalent (molecular)

c)

Metallic

d)

Network covalent

113.

The molecules in an unknown substance are very weakly attracted to each other. What is the bonding type for this substance?

a)

Nonpolar covalent (molecular)

b)

Ionic

c)

Metallic

d)

Polar covalent (molecular)

114.

Why do nonpolar substances tend to be gases and not liquids or solids?

a)

They have only weak London dispersion forces, making them easy to separate into gas.

b)

They have strong ionic attractions that keep particles far apart.

c)

They form extensive hydrogen-bonded networks that trap them as gases.

d)

Metallic bonding causes electrons to move freely, producing gases.

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10th Grade

Final exam first semester

111 questions

Final exam first semester

quiz

Worksheet

•

9th - 12th Grade