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Chemistry S1 Final Exam Review

Total questions: 80

Worksheet time: 1hrs 21mins

Name
Class
Date
1.

Which statement correctly defines atomic number?

a)

Total count of protons and neutrons

b)

Number of protons in the nucleus

c)

Number of electrons in neutral atoms

d)

Average mass of all isotopes

2.

A K+ ion has 19 protons and 18 electrons. What is its net charge?

a)

+1 charge overall

b)

−1 charge overall

c)

+2 charge overall

d)

0 charge overall

3.

201Hg2+ has 80 protons, 78 electrons, and mass number 201. Which description is accurate?

a)

Mercury cation with normal mass

b)

Mercury cation and also an isotope

c)

Neutral mercury with mass number 201

d)

Mercury anion but not an isotope

4.

An ion of iodine written as I− has 53 protons and 54 electrons. Which term classifies it?

a)

Neutral iodine atom

b)

Isotope with +1 charge

c)

Anion with −1 charge

d)

Cation with −1 charge

5.

Nickel written as 60Ni has 28 protons and 32 neutrons. What does the superscript 60 indicate?

a)

The charge on the nickel ion

b)

The atomic number of nickel

c)

The number of electrons present

d)

The mass number for this isotope

6.

Neon has atomic number 10 and atomic mass 20 with charge 0. How many neutrons are in this neon atom?

a)

0 neutrons total

b)

20 neutrons total

c)

10 neutrons total

d)

10 neutrons fewer than protons

7.

Which pair of counts leads to a neutral atom?

a)

Protons equal electrons

b)

Protons equal neutrons

c)

Electrons exceed neutrons

d)

Protons exceed electrons by one

8.

Match each species to its classification.

a)

K+

1.

cation

b)

I−

2.

anion

c)

Sr2+

3.

cation

d)

60Ni

4.

isotope

9.

An atom of carbon-13 has 6 protons and 7 neutrons. What makes it an isotope of carbon?

a)

Different number of protons than carbon

b)

Different number of neutrons than carbon

c)

Different number of energy levels

d)

Different number of electrons than carbon

10.

Titanium written as 46Ti has atomic number 22 and 24 neutrons. Which conclusion fits these data?

a)

It is a titanium isotope

b)

It is neutral but not an isotope

c)

It is a titanium anion

d)

It is a titanium cation

11.

What is the key difference between an ion and an isotope?

a)

Ions have charge, isotopes have different mass number

b)

Ions have extra neutrons, isotopes have extra electrons

c)

Ions change atomic number, isotopes change charge

d)

Ions are neutral, isotopes are always charged

12.

Iron shown as 59Fe3+ has 26 protons, 23 electrons, and 33 neutrons. Which statement is correct?

a)

It is both a cation and an isotope

b)

It is a neutral iron atom

c)

It is only a cation of iron

d)

It is only an isotope of iron

13.

Which balanced equation shows hydrogen reacting with oxygen to form water with correct stoichiometric coefficients?

a)

2 H2 + 2 O2 → 2 H2O

b)

1 H2 + 2 O2 → 2 H2O

c)

2 H2 + 1 O2 → 2 H2O

d)

H2 + O2 → H2O

14.

Ammonia decomposes to nitrogen and hydrogen. Which set of coefficients balances NH3 → N2 + H2?

a)

1, 1, 2

b)

3, 2, 1

c)

2, 2, 2

d)

2, 1, 3

15.

Magnesium reacts with nitrogen to form magnesium nitride. What coefficients balance Mg + N2 → Mg3N2?

a)

2, 1, 3

b)

1, 1, 1

c)

3, 1, 1

d)

3, 2, 1

16.

Silver(I) oxide breaks down to silver and oxygen. Choose the correctly balanced equation.

a)

Ag2O → Ag + O2

b)

2 Ag2O → 4 Ag + 1 O2

c)

2 Ag2O → 2 Ag + 2 O2

d)

Ag2O → 4 Ag + 1 O2

17.

Aluminum reacts with oxygen to form aluminum oxide. Which coefficients balance Al + O2 → Al2O3?

a)

2, 3, 1

b)

4, 3, 2

c)

3, 2, 4

d)

1, 1, 1

18.

Glucose synthesis: CO2 + H2O → C6H12O6 + O2. What coefficient must be placed before CO2 to balance the equation?

a)

12

b)

6

c)

5

d)

4

19.

Identify the correctly balanced equation for sodium bromide reacting with calcium fluoride.

a)

2 NaBr + 2 CaF2 → 2 NaF + CaBr2

b)

NaBr + 2 CaF2 → NaF + CaBr2

c)

2 NaBr + CaF2 → 2 NaF + CaBr2

d)

NaBr + CaF2 → NaF + CaBr2

20.

Balancing H2S + Cl2 → S8 + HCl requires accounting for sulfur atoms. What is the correct coefficient before H2S?

a)

4

b)

16

c)

8

d)

1

21.

Which statement best defines a chemical formula?

a)

Pictures illustrating molecular shapes

b)

Names describing elements in words

c)

Balanced numbers in an equation

d)

Symbols showing atoms in a substance

22.

What does a chemical equation represent?

a)

Masses of atoms in a sample

b)

Formulas for reactants and products

c)

Rules for naming ionic compounds

d)

Steps for separating mixtures

23.

In a chemical reaction, what are reactants?

a)

Smallest unit of any matter

b)

Substances formed after reaction

c)

Two or more atoms bonded

d)

Substances present before reaction

24.

Which description fits products in a reaction?

a)

Atoms within a single element

b)

Substances placed on left side

c)

Liquids forming a precipitate

d)

Substances created by the reaction

25.

What is the smallest unit of matter?

a)

Atom

b)

Molecule

c)

Element

d)

Compound

26.

Which term describes a substance made of only one type of atom?

a)

Molecule

b)

Mixture

c)

Compound

d)

Element

27.

What is a molecule?

a)

Two or more atoms chemically bonded

b)

A substance made of molecules overall

c)

A single atom in a crystal lattice

d)

The left side of a chemical equation

28.

Which statement defines a compound?

a)

A single atom of any element

b)

Two unrelated substances mixed

c)

An equation showing mass changes

d)

A substance made up of molecules

29.

Which is a valid sign that a chemical reaction has occurred?

a)

Temperature change is observed

b)

Container label is different

c)

Atoms visibly become larger

d)

Equation includes more symbols

30.

Which observation indicates precipitate formation?

a)

Light is absorbed by solution

b)

Product is a different color

c)

Solids form from liquid reactants

d)

Gas bubbles dissolve completely

31.

Gas production can be a sign of reaction. Which example fits?

a)

Reactants are written in italics

b)

Beaker shape looks different

c)

Mass reading on scale increases

d)

Bubbles appear in the mixture

32.

Which statement summarizes the law of conservation of mass?

a)

Atoms disappear when gas is produced

b)

Matter is not created or destroyed

c)

Energy becomes matter in reactions

d)

Mass always decreases during heating

33.

Why must chemical equations be balanced?

a)

To reduce the number of atoms

b)

To show mass is conserved

c)

To make formulas identical

d)

To keep products on the left

34.

Which statement best defines an element?

a)

Blend with visible separate parts

b)

Substance made of bonded molecules

c)

Blend with uniform appearance throughout

d)

Substance made of one type of atom

35.

Which example represents a compound?

a)

Oxygen gas molecules

b)

Table salt sodium chloride

c)

Latte of coffee with milk

d)

Fresh garden salad

36.

Which description fits a homogeneous mixture?

a)

Chemically bonded different atoms

b)

Pure substance with one atom type

c)

Mixture with unequal distribution

d)

Uniform mixture with no visible parts

37.

Which is a heterogeneous mixture?

a)

Air evenly mixed gases

b)

Alloy with uniform composition

c)

Salt solution dissolved fully

d)

Salad with distinct components

38.

What is mass measured with in typical lab practice?

a)

Calorimeter apparatus

b)

Balance measuring scale

c)

Thermometer instrument

d)

Graduated cylinder device

39.

Which statement defines volume?

a)

Amount of matter present

b)

Ability to react chemically

c)

Amount of space occupied

d)

Ratio of mass to volume

40.

Density is best expressed as which relationship?

a)

Mass times volume product

b)

Mass plus volume combined

c)

Mass divided by volume

d)

Volume divided by mass

41.

Which is a chemical property?

a)

Density of a sample

b)

Color of a metal

c)

Reactivity with acids

d)

Electrical conductivity

42.

Which is a physical property?

a)

Malleability of metal

b)

Acid-base neutralization

c)

Tendency to corrode

d)

Flammability in oxygen

43.

Water has a density of approximately 1.0 g/cm³. Which statement is consistent with this value?

a)

One liter has mass near one kilogram

b)

One gram occupies ten cubic centimeters

c)

One milliliter has mass near one gram

d)

One cubic meter has mass one gram

44.

A student measures a block with mass 60 grams and volume 20 mL. What is its density?

a)

4.0 g/mL value

b)

1.5 g/mL value

c)

2.0 g/mL value

d)

3.0 g/mL value

45.

A rock has mass 225 grams. In a graduated cylinder, water rises from 50.0 mL to 75.0 mL after adding the rock. What is the rock’s density?

a)

7.5 g/mL value

b)

9.0 g/mL value

c)

10.0 g/mL value

d)

22.5 g/mL value

46.

Two rulers give measurements: 2.35 cm ± 0.02 cm and 2.4 cm ± 0.1 cm for the same object. Which statement best explains the difference?

a)

Different parallax increases actual value

b)

Different zero errors change true length

c)

Different resolution yields different uncertainty

d)

Different temperature alters metal length

47.

Match each instrument to its primary measurement.

a)

Ruler

1.

Length

b)

Graduated cylinder

2.

Liquid volume

c)

Thermometer

3.

Temperature

d)

Triple beam balance

4.

Mass

48.

Which practice minimizes error when reading a meniscus in a graduated cylinder?

a)

Stand two meters away

b)

Align eyes with meniscus level

c)

View at an angle from the side

d)

Hold cylinder above eye level

49.

Convert 10 centimeters to millimeters.

a)

1000 mm

b)

1 mm

c)

100 mm

d)

10 mm

50.

How many meters are in 2 kilometers?

a)

200 m

b)

2000 m

c)

0.2 m

d)

20 m

51.

Convert 3.5 meters to centimeters.

a)

3.5 cm

b)

35 cm

c)

3500 cm

d)

350 cm

52.

Convert 2000 millimeters to meters.

a)

2 m

b)

20 m

c)

200 m

d)

0.2 m

53.

Convert 600 meters to kilometers.

a)

0.6 km

b)

6 km

c)

0.06 km

d)

60 km

54.

Convert 110 meters to centimeters.

a)

110 cm

b)

1100 cm

c)

11,000 cm

d)

1,100,000 cm

55.

Convert 943 centimeters to millimeters.

a)

943 mm

b)

9.43 mm

c)

9430 mm

d)

94.3 mm

56.

Convert 204000 meters to kilometers.

a)

0.204 km

b)

2.04 km

c)

20.4 km

d)

204 km

57.

Convert 155 millimeters to centimeters.

a)

155 cm

b)

0.155 cm

c)

15.5 cm

d)

1.55 cm

58.

Convert 4.8 kilometers to meters.

a)

480 m

b)

48 m

c)

4800 m

d)

48,000 m

59.

Convert 3.5 centimeters to millimeters.

a)

35 mm

b)

3.5 mm

c)

350 mm

d)

0.35 mm

60.

Recall the formula for percent error when comparing an experimental value to an actual value.

a)

(experimental+actual)/actual×100%

b)

(actual−experimental)/actual×100%

c)

(actual−experimental)/experimental×100%

d)

(experimental−actual)/actual×100%

61.

An object’s actual mass is 50 kg. A balance reads 48 kg. What is the percent error?

a)

4%

b)

8%

c)

2%

d)

6%

62.

Boiling water has an actual temperature of 100°C. A student’s experimental reading is 94°C. Calculate the percent error.

a)

4%

b)

5%

c)

7%

d)

6%

63.

To find density, you ​divide ​ (a)   by ​ (b)  

Choose from the below words
mass
volume
density
distance
64.
Is burning wood a chemical or physical change?
a)
chemical
b)
physical
65.

This picture represents which of the following?

a)

element

b)

compound

66.

What are the products of the chemical reaction pictured?

a)

CH4 and CO2

b)

CH4 and O2

c)

CO2 and H2O

d)

O2 and H2O

67.

Given the following reading a the triple beam balance, what is the mass of the object on the balance? Include units

(a)  

68.

Record the volume.

_______ mL

4 lines
69.
a)
Student A
b)
Student B
c)
Student C
d)
Cannot be determined
70.

Solutions that have more OH– ions than H+ ions are

a)

acids

b)

bases

c)

enzymes

d)

neutral

71.

Solutions that have more H+ ions than OH- ions are

a)

acids

b)

bases

c)

enzymes

d)

neutral

72.

Which of the following is the strongest acid?

a)

soap - 10

b)

HCL - 0

c)

blood - 7.45

d)

soft drink - 3

73.

Which of the following is the strongest base?

a)

soap - 10

b)

HCL - 0

c)

blood - 7.45

d)

soft drink - 3

74.

Which of these pH values represent an acid?

a)

4

b)

8

c)

10

d)

12

75.

Milk is a very weak acid. What might its pH value be?

a)

6.5

b)

7.8

c)

4.2

d)

12.2

76.

Which of the following are properties of acids?

a)

They conduct electricity when dissolved in water

b)

They taste sour

c)

They react with metals to produce hydrogen gas

d)

All of the answer choices are correct

77.

Which of the following is a property of a base?

a)

bitter taste

b)

reacts with metals

c)

salty

d)

sour taste

78.

Bases have many uses. They are mainly used to make

a)

cleaning products

b)

soaps

c)

concrete

d)

all of the answer choices

79.

Which salt is formed in a reaction between HBr and LiOH?

a)

LiBr

b)

BrLi

c)

NaCl

d)

NaOH

80.

In a water solution, how do acids differ from bases?

a)

Acids form salts, but bases do not

b)

Acids turn litmus blue, while bases turn litmus red

c)

Acids form hydrogen ions (H+), while bases form hydroxide ions (OH-)

d)

Bases form salts, but acids do not

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