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Physical Science Semester B Practice Test

Total questions: 55

Worksheet time: 28mins

Name
Class
Date
1.

Mendeleev arranged the elements in his periodic table in order of...

a)

Atomic number

b)

number of electrons

c)

Atomic mass

d)

Number of Neutrons

2.

Mendeleev's decision to leave gaps in his periodic table was supported by the discovery of....

a)

Electrons

b)

Protons

c)

Carbon

d)

Gallium

3.

An arrangement of elements into columns, based on a set of properties that repeat from row to row is called a(n)

a)

Group

b)

Column

c)

Periodic Table

d)

Periodic Arrangement

4.

Which of the following types of information did Mendeleev NOT know about each element?

a)

Name of the element

b)

Number of protons

c)

Relative Mass

d)

Physical Properties

5.

Mendeleev used the properties of elements located near the blank spaces within his periodic table to predict properties of undiscovered elements.

a)

True

b)

False

6.

In the modern periodic table, elements are arranged in order of....

a)

Increasing Atomic Mass

b)

Decreasing Atomic Mass

c)

Increasing Atomic Number

d)

Decreasing Atomic Number

7.

A row of the periodic table is called a(n)

a)

Group

b)

Grouping

c)

Period

d)

Trend

8.

A column on the periodic table is called a(n)

a)

Group

b)

Period

c)

Trend

d)

Task

9.

The atomic mass of an element is determined by...

a)

The distribution of an elements isotopes in nature and the masses of those isotopes

b)

The number of protons and electron in the nucleus of an atom

c)

The distribution of an atoms protons in nature

d)

The desire for an element to achieve a stable octet

10.

Using your periodic table, determine the atomic mass of Beryllium.

a)

2

b)

4

c)

5

d)

9

11.

Using your periodic table, determine the atomic number of Magnesium.

a)

12

b)

24

c)

36

d)

48

12.

Using your periodic table, determine the number of neutrons for Beryllium

a)

4

b)

5

c)

9

d)

13

13.

Which of the following classes of elements are most common on the periodic table?

a)

Metals

b)

Nonmetals

c)

Metalloids

14.

Using your periodic table, which of the following elements is considered a metalloid?

a)

Silicon

b)

Iodine

c)

Osmium

d)

Mercury

15.

Noble gasses are made up of which of the following classes of elements?

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Not enough information to answer the question

16.

elements in a group have similar properties because they have...

a)

The same metallic properties

b)

The same number of protons

c)

The same number of valence electrons

d)

The same number of neutrons

17.

Based on it's location on the periodic table, which of the following elements is MOST reactive?

a)

Magnesium

b)

Sodium

c)

Aluminum

d)

Silicon

18.

Which of the following elements falls under the alkali Earth metal group?

a)

Sodium

b)

Nitrogen

c)

Strontium

d)

Chlorine

19.

Based on their location on the periodic table, which class of elements is most likely to lose electrons when bonding?

a)

Metals

b)

Nonmetals

c)

Metalloids

20.

Using your periodic table, determine how many valence electrons does the element Boron have?

a)

1

b)

2

c)

3

d)

4

21.

Which of the following groups of the periodic table are the least reactive?

a)

Alkali Metals

b)

Alkali Earth Metals

c)

Halogens

d)

Noble Gases

22.

Which of the following is the correct name for the compound listed below?

KBr

a)

Bromine Potassium

b)

Potassium Bromide

c)

Potassium Bromine

d)

No idea

23.

Which of the following is the correct name for the compound listed below?


AlBr3

a)

Aluminum Bromine

b)

Aluminum Bromide

c)

Bromine Aluminide

d)

Bromine aluminum

24.

Determine the correct formula for the following compound:


Magnesium Chloride

a)

MgCl

b)

ClMg

c)

MgCl2

d)

Mg2Cl

25.

Determine the correct formula for the compound listed below:


Potassium Sulfide

a)

KS

b)

SK

c)

K2S

d)

KS2

26.

Determine whether the following statement is true or false:


Molecular substances generally have low melting points

a)

True

b)

False

27.

Determine whether the following statement is true or False:


Molecular substances form compounds by sharing electrons between atoms.

a)

True

b)

False

28.

Determine if the following compound is ionic or covalent.


Iron (II) Oxide

a)

Ionic

b)

Covalent

29.

Determine if the following compound is ionic or covalent


Sulfur Tetrachloride

a)

Ionic

b)

Covalent

30.

Name the following compound:


N2O3

a)

Nitrogen Oxide

b)

Dinitrogen Diooxide

c)

Dinitrogen Trioxide

d)

Trinitrogen Dioxide

31.

Name the following compound:


CS2

a)

Monocarbon Disulfide

b)

Dicarbon Disulfide

c)

Carbon Disulfide

d)

Carbon Sulfide

32.

Write the formula of the following compound:

Carbon Tetrachloride

a)

CCL

b)

CCl

c)

C4Cl

d)

CCl4

33.

Write the formula for the following compound:

Dihydrogen Monoxide

a)

HO

b)

H2O2

c)

H2O

d)

O2H

34.

A metal is an element or compound with high ___________

a)

electrical conductivity

b)

foldability

c)

bendability

d)

elasticity

35.

Which of the following types of bonds form between two metals?

a)

Metallic Bond

b)

Ionic bond

c)

Covalent Bond

d)

James Bond

36.

The sea of delocalized electrons and the attraction to all of the positive ions is the metallic bond, which holds the entire metallic structure together.

a)

True

b)

False

37.

If a metal rod wrapped in paper is placed in a flame, will it catch on fire?

a)

Yes, the paper will burn

b)

No, because the energy from the flame is easily distributed to the metal.

38.

Which of the following terms best fits the description below?

The property of a material that indicates its ability to conduct heat

a)

Delocalized

b)

Malleability

c)

Thermal Conductivity

d)

Luster

39.

Which of the following elements is most likely to give up electrons when bonding?

a)

Calcium

b)

Oxygen

c)

Silicon

d)

Bromine

40.

Based on the element provided, which is most likely to become an ANION?

a)

Sodium

b)

Fluorine

c)

Neon

d)

Aluminum

41.

Which of the following is NOT a property of an ionic compound?

a)

Maintains strong attractions among ions within the crystal lattice

b)

Maintains a high melting point

c)

In its solid state, it is a poor conductor of electricity

d)

Bonds are very weak and form from a sharing of electrons

42.

Which of the following types of covalent compounds does NOT share electrons equally?

a)

Diatomic Molecules

b)

Non-polar Molecules

c)

Polar Molecules

43.

Which of the following ionic compounds contains a transition metal?

a)

Potassium Permanganate

b)

Sodium Chloride

c)

Iron (III) Oxide

d)

Sodium Hydroxide

44.

Metals conduct heat well because of the sea of delocalized electrons.

a)

True

b)

False

45.

Which of the following is considered a reactant in the equation below:


Carbon Dioxide + Water --> Sugar + Oxygen gas

a)

Water

b)

Sugar

c)

Oxygen Gas

d)

Both sugar and oxygen gas

46.

you can balance a chemical equation by changing the __________

a)

Subscript

b)

Elements

c)

Coefficient

d)

Yield

47.

A new substance that forms from a chemical reaction is called a(n)

a)

Reactant

b)

Product

c)

Yield

d)

Coefficient

48.

Determine whether the following statement is true or false:


Mass cannot be created nor destroyed in a chemical reaction

a)

True

b)

False

49.

In the following chemical formula, how many magnesium atoms are in the compound?


2MgCl2

a)

1

b)

2

c)

3

d)

4

50.

Determine which of the following answers is the correct balanced equation for the skeleton equation listed below:

Al2O3 --> Al + O2

a)

Al2O3 --> Al + O2

b)

4 Al2O3 --> 3 Al + 2O2

c)

AlO --> Al + O

d)

2 Al2O3 --> 4 Al + 3 O2

51.

Determine which of the following answers is the correct balanced equation for the skeleton equation listed below:

P + O2 --> P2O5

a)

2P + O2 --> P2O5

b)

P + 3O2 --> 4P2O5

c)

4P + 5O2 --> 2P2O5

d)

P + O2 --> P2O5

52.

What type of reaction is shown in the example below:


P + O2 --> P2O5

a)

Decomposition

b)

Synthesis

c)

Combustion

d)

Single Replacement

53.

What type of reaction is shown in the chemical equation below?


BaCl2 + H2SO4 --> BaSO4 + HCl

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

54.

What type of reaction is shown in the example formula shown below:


KClO3 --> KCl + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

55.

A reaction such as the burning of methane gas is an example of a(n) __________________reaction.

a)

endothermic

b)

exothermic

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