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IASE 8th Grade Midterm Study Guide

Total questions: 188

Worksheet time: 2hrs 43mins

Name
Class
Date
1.

The investigation & exploration of natural events & of the new information that results from these investigations.

a)

hypothesis

b)

science

c)

theory

d)

observation

2.

the act of using one or more of your senses to gather information & taking note of what occurs.

a)

hypothesis

b)

science

c)

observation

d)

theory

3.

a logical explanation of an observation that is drawn from prior knowledge

a)

prediction

b)

science

c)

observation

d)

inference

4.

a possible explanation for an observation that can be tested by scientific investigations.

a)

hypothesis

b)

theory

c)

science

d)

prediction

5.

a statement of what will happen next in a sequence of events

a)

science

b)

inference

c)

hypothesis

d)

prediction

6.

the practical use of scientific knowledge, especially for industrial or commercial use

a)

science

b)

technology

c)

observation

d)

theory

7.

an explanation of observations or events that is based on knowledge gained from many observations & investigations.

a)

observation

b)

hypothesis

c)

scientific theory

d)

scientific law

8.

a rule that describes a pattern in nature.

a)

scientific theory

b)

scientific law

c)

hypothesis

d)

observation

9.

any factor that can have more than one value.

a)

prediction

b)

variable

c)

science

d)

critical thinking

10.

the factor you want to test

a)

independent variable

b)

dependent variable

c)

variable

d)

experiment

11.

the factor you observe or measure during an experiment

a)

independent variable

b)

dependent variable

c)

experiment

d)

science

12.

the factors in an experiment that remain the same

a)

variable

b)

constants

c)

dependent variable

d)

independent variable

13.

used to study how a change in the independent variable changes the dependent variable

a)

experimental group

b)

control group

c)

variable

d)

constant

14.

contains the same factors as the experimental group, but the independent variable is not changed.

a)

experimental group

b)

variable

c)

control group

d)

constant

15.

uses words to describe observation

a)

qualitative data

b)

quantitative data

c)

constant

d)

variable

16.

uses numbers to describe an observation

a)

qualitative data

b)

quantitative data

c)

variable

d)

constant

17.

the smallest piece of an element that still represents that element.

a)

atom

b)

molecule

c)

substance

d)

mixture

18.

most of an atom's mass and a positive charge is found in this area

a)

neutron

b)

nucleus

c)

proton

d)

electron

19.

atomic particles and their charges

a)

proton +1, neutron 0, electron -1

b)

neutron + 1, proton 0, electron -1

c)

photon +1, neutron 0, electron -1

d)

proton +1, neutron 0, electrode -1

20.

an area around an atomic nucleus where an electron is most likely to be located

a)

circular orbit

b)

nucleus

c)

electron cloud

d)

the library

21.

the number of protons in an atom of an element

a)

atomic mass

b)

atomic number

c)

isotope

d)

ion

22.

atoms of the same element that have different numbers of neutrons

a)

isotope

b)

isomer

c)

ion

d)

molecule

23.

sum of number of protons & neutrons in an atom

a)

isotope

b)

ion

c)

atomic number

d)

mass number

24.

average mass of an element's isotopes, weighted according to their abundance

a)

mass number

b)

atomic number

c)

average atomic mass

d)

ion

25.

a process that occurs when an unstable atomic nucleus changes into a more stable nucleus by emitting radiation

a)

radioactive decay aka nuclear decay

b)

readiosmactive decay

c)

knuckular decay

d)

albatross

26.

an atom that is no longer neutral because it has gained or lost electrons

a)

ion

b)

isotope

c)

isomer

d)

molecule

27.

A force that holds two or more atoms together

a)

chemical bond

b)

physical bond

c)

valence shell

d)

nucleus

28.

matter that is made up of two or more different kinds of atoms joined together by chemical bonds.

a)

mass

b)

compound

c)

quarks

d)

neutrons

29.

a force that holds two or more bonds together

a)

elmer's glue

b)

chemical bond

c)

physical bond

d)

hydrocarbon

30.

electrons closest to the nucleus

a)

have the least amount of energy

b)

have the greatest amount of energy

c)

can not exceed 8

d)

can not exceed 4

31.

atoms are most stable when they contain 8 electrons in the

a)

outermost valence shell

b)

innermost shell

c)

orbit around the nucleus

d)

molecule

32.

atoms are most stable when they have 8 electrons in their outermost shell

a)

the valence shell rule

b)

the rule of Octet

c)

noble gas rule

d)

covalent bonding

33.

the outermost layer of electrons in an atom that participate in chemical bonding

a)

covalent bonding

b)

ionic bonding

c)

valence shell

d)

functional group

34.

The dots in electron dot diagrams represent

a)

all electrons in an atom

b)

all valence shell electrons in an atom

c)

protons in an atom

d)

all subatomic particles in an atom

35.

Who invented the Electron Dot Diagram method?

a)

Gilbert Lewis

b)

Antoine Lavoisier

c)

JJ Thomson

d)

Ernest Rutherford

36.

An electron dot diagram is shown for Nitrogen. How many bonds can it form?

a)

5

b)

3

c)

4

d)

1

37.

How would you describe atoms that between 1-7 electrons in their valence shell?

a)

unreactive

b)

reactive

c)

noble gases

d)

alkali metals

38.

The elements in group 18 are called

a)

Noble Gases

b)

Alkali Metals

c)

Alkaline Metals

d)

Halogens

39.

What term would you use to describe Neon?

a)

Noble Gas

b)

Chemically Stable

c)

Unreactive

d)

All of these

40.
Pure forms of these elements are stored in oil so they won't react with oxygen and water in the air.
a)
Alkali Metals
b)
Alkaline-earth metals
c)
Halogens
d)
Noble Gases
41.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
42.
This class of elements are sometimes called "semiconductors."
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Groups
43.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
44.
The yellow atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
45.
Group 18 elements are known as the _____ _____ and have full valence shells.
a)
royal gases.
b)
supreme solids.
c)
noble gases.
d)
legit liquids.
46.
Elements in the same ________ are more chemically similar.
a)
group
b)
period
c)
club
d)
table
47.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
48.

The Periodic Table is a chart of the elements arranged into ______ and _________ according to their physical & chemical properties

a)

groups and periods

b)

solid and liquid

c)

solids, liquids and gases

d)

solids and gases

49.

Dmetri Mendeleev studied these four characteristics of elements

a)

Density; Color; Melting Point; Atomic Mass

b)

Density, Color, Boiling Point; Atomic Mass

c)

Density; Color; Melting Point; Atomic Bass

d)

Density; Color; Boiling Point; Atomic Number

50.

"Periodic" means

a)

organized

b)

happens rarely

c)

happens occasionally

d)

repeating pattern

51.

What would you find in the upper right corner of the periodic table?

a)

metalloids

b)

nonmetals

c)

metals

d)

alkali metals

52.

This scientist made some corrections to the periodic table

a)

Henry Moseley

b)

Dmetri Mendeleev

c)

Ernest Rutherford

d)

JJ Thomson

53.

What change did Henry Moseley make to Mendeleev's periodic table

a)

Switched it from order of atomic number to atomic mass

b)

Switched it from order of atomic mass to atomic number

c)

Switched it to exclude ions

d)

Added isotopic forms

54.

the rows on the periodic table

a)

columns

b)

periods

c)

groups

d)

noble gases

55.

Patterns in a group include :

a)

freezing point & valence shell electrons

b)

density only

c)

density, melting point & boiling point

d)

boiling point only

56.

A column on the periodic table

a)

group

b)

period

c)

row

d)

metalloids

57.

Patterns in a group include :

a)

freezing point & valence shell electrons

b)

density only

c)

density, melting point & boiling point

d)

boiling point only

58.

this group of elements has one electron in their valence shell that they love to give away in explosive reactions with water

a)

halogens

b)

noble gases

c)

nonmetals

d)

alkali metals

59.

Group 17 elements often have 7 electrons in their valence shell and love to take electrons from Group 1 and are called

a)

noble gases

b)

halogens

c)

alkali metals

d)

metalloids

60.

These elements conduct electricity very well

a)

metalloids

b)

metals

c)

nonmetals

d)

noble gases

61.

most of an atom's mass and a positive charge is found in this area

a)

neutron

b)

nucleus

c)

proton

d)

electron

62.

A chemical bond formed when two atoms share one or more pairs of valence electrons.

a)

ionic bond

b)

covalent bond

c)

bond line formula

d)

structural formula

63.

exists when one pair of electrons is shared by two atoms

a)

single covalent bond

b)

double covalent bond

c)

single ionic bond

d)

double ionic

64.

exists when two atoms share two pairs of electrons

a)

double covalent bond

b)

double ionic bond

c)

single covalent bond

d)

single ionic bond

65.

Which displays the correct order of bond strength?

a)

triple bonds < double bonds < single bonds

b)

single bonds > triple bonds > double bonds

c)

single bonds > double bonds > triple bonds

d)

triple bonds > double bonds > single bonds

66.

Nonmetals are more likely to

a)

form covalent bonds with other nonmetals

b)

form covalent bonds with metals

c)

form ionic bonds with other nonmetals

d)

be hard and not brittle

67.

Characteristics of covalent nonmetals

a)

high melting & high boiling points

b)

low melting & low boiling points

c)

Usually solid at room temperature

d)

Usually form ionic bonds with other nonmetals

68.

These make good insulators, which means they are bad conductors of heat & electricity

a)

metals

b)

nonmetals

c)

transition metals

d)

alkaline earth metals

69.

A group of atoms held together by covalent bonding that acts as an independent unit

a)

element

b)

molecule

c)

bacteria

d)

cell

70.

A molecule that has a partial positive end & a partial negative end because of unequal sharing of electrons

a)

polar molecule

b)

nonpolar molecule

c)

element

d)

cell

71.

Describe what is happening in this photo

a)

It is a nonpolar molecule with unequal distribution of electrons

b)

It is a polar molecule with unequal distribution of electrons

c)

It is a water molecule with ionic bonding

d)

It is a polar molecule equal distribution of electrons

72.

What would happen if you put polar and nonpolar molecules together?

a)

they have an explosive reaction

b)

they will not mix

c)

the polar will be dissolved in the nonpolar

d)

the nonpolar will be dissolved in the polar

73.

what would generally happen if you mix two polar molecules together?

a)

they will not mix

b)

they will mix and one will dissolve in the other

c)

they will have an explosive reaction

d)

they will create a heterogeneous mixture

74.

a group of chemical symbols and numbers that represent the elements and the number of atoms of each element that make up a compound.

a)

periodic formula

b)

bond line formula

c)

chemical formula

d)

structural formula

75.

What is the general term for this model of a molecule?

a)

structural formula

b)

bond line formula

c)

chemical formula

d)

dot diagram

76.

What is the general name of this model of a molecule?

a)

chemical formula

b)

structural formula

c)

electron dot diagram

d)

bond line formula

77.

What is the name of this type of model of a molecule?

a)

chemical formula

b)

bond line formula

c)

structural formula

d)

ball and stick formula

78.

What model of a molecule does this picture represent?

a)

ball and stick formula

b)

space filling formula

c)

chemical formula

d)

structural formula

79.

A water molecule is polar because

a)

the shared electrons are pulled closer to the Oxygen atom than the Hydrogen atoms

b)

the shared electrons are pulled closer to the Hydrogen atom than the Oxygen atoms

c)

the shared electrons are pulled farther away from the Oxygen atom than the Hydrogen atoms

d)

the shared electrons are pulled farther away from the Hydrogen atom than the Oxygen atoms

80.

Carbon Dioxide is nonpolar because

a)

the shared electrons are equally distributed

b)

the shared electrons are not equally distributed

c)

the electrons are not shared

d)

the electrons are destroyed

81.

A polar molecule's valence electrons are

a)

equally distributed

b)

not equally distributed

c)

destroyed

d)

equal distances apart

82.

An atom that is no longer electrically neutral because it has lost or gained valence electrons.

a)

isotope

b)

ion

c)

isomer

d)

noble gas

83.

an ion with a positive charge

a)

anion

b)

cation

c)

isotope

d)

isomer

84.

an ion with a negative charge

a)

anion

b)

cation

c)

isotope

d)

isomer

85.

a bond between a metal and a nonmetal

a)

ionic bond

b)

covalent bond

c)

metallic bond

d)

hydrogen bond

86.

Sodium and Chlorine atoms bonding together is an example of a

a)

metallic bond

b)

covalent bond

c)

ionic bond

d)

hydrogen bond

87.

Electrons are taken or lost, but not shared

a)

metallic bond

b)

covalent bond

c)

ionic bond

d)

hydrogen bond

88.

A bond between a nonmetal and a nonmetal

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

hydrogen bond

89.

A bond between a metal and a metal

a)

hydrogen bond

b)

ionic bond

c)

covalent bond

d)

metallic bond

90.

metal atoms typically

a)

share valence electrons

b)

gain valence electrons

c)

lose valence electrons

d)

make valence electrons

91.

nonmetal atoms typically

a)

lose electrons

b)

gain electrons

c)

share electrons

d)

make electrons

92.

the attraction between positive and negative ions in an ionic compound

a)

ionic bond

b)

metallic bond

c)

covalent bond

d)

hydrogen bond

93.

ionic compounds have relatively

a)

high melting and boiling points

b)

high melting points

c)

high boiling points

d)

low melting and boiling points

94.

water that contains dissolved ionic compounds is a good

a)

insulator

b)

conductor

c)

metallic bond

d)

noble gas

95.

Your friend attempts to light a light bulb using salt water as a conductor. What do you tell him/her?

a)

Ya nuts?

b)

Water is an insulator!

c)

That's impossible!

d)

It! Just! Might! Work!

96.

When nonmetal ions bond to metal ions there are

a)

molecules

b)

no molecules

c)

covalent bonds

d)

metallic bonds

97.

Bond formed when many metal atoms share their pooled valence electrons

a)

covalent bonding

b)

metallic bonding

c)

ionic bonding

d)

hydrogen bonding

98.

Metallic bonding involves

a)

taken or lost electrons

b)

shared electrons

c)

free flowing electrons

d)

no electrons

99.

bonding between aluminum atoms causes

a)

the aluminum to become positive ions

b)

electrons to freely flow around aluminum atoms

c)

a "sea of electrons" to form

d)

all of these

100.

the ability of metal to be shaped and bent without breaking

a)

ductility

b)

malleability

c)

luster

d)

conductivity

101.

the ability of metals to be pulled into thin wires

a)

ductility

b)

malleability

c)

conductivity

d)

luster

102.

the ability of metals to reflect light

a)

luster

b)

ductility

c)

malleability

d)

conductivity

103.

Almost always solid at room temperature

a)

metals

b)

nonmetals

c)

gases

d)

olive oil

104.

This metal is the only metal to be liquid at room temperature

a)

gallium

b)

mercury

c)

aluminum

d)

sodium

105.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
106.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
107.

What would a superscript of +2 on the abbreviation O tell you?

a)

Oxygen with 2 missing electrons

b)

Oxygen with 2 extra electrons

c)

Oxygen that is an anion

d)

Two Oxygen atoms

108.

When abbreviating ions, we write the number with a plus or minus before it

a)

Above the abbreviation & to the right

b)

Below the abbreviation & to the left

c)

Before the abbreviation

d)

Above the abbreviation

109.

This type of change does not produce new substances.

a)

Physical change

b)

Chemical change

c)

Le Chatelier's Principle

d)

Redox reaction

110.

Ice melts and becomes liquid water.

a)

physical change

b)

chemical change

c)

sublimation

d)

evaporation

111.

one or more substances change into new substances.

a)

physical change

b)

chemical change

c)

evaporation

d)

condensation

112.

A chemical change is also known as

a)

sublimation

b)

a physical change

c)

a chemical reaction

d)

condensation

113.

A process in which atoms of one or more substances rearrange to form one or more new substances.

a)

sublimation

b)

physical reaction

c)

chemical reaction

d)

condensation

114.

changes in properties such as change in color, odor, formation of bubbles, & formation of precipitate are all signs of a

a)

possible chemical reaction

b)

sublimation

c)

definite chemical reaction

d)

condensation

115.

energy changes, such as changes in light, sound, & temperature are indicative of

a)

definite chemical change

b)

condensation

c)

possible chemical change

d)

sublimation

116.

Which of the following are true in regards to chemical reactions

a)

new bonds are formed in reactants

b)

bonds in reactants are broken

c)

bonds in products are broken

d)

all of these

117.

Which of the following are true in regards to chemical reactions

a)

new bonds are formed in reactants

b)

bonds in products are formed

c)

bonds in products are broken

d)

all of these

118.

a description of a reaction using element symbols & chemical formulas

a)

physical change

b)

chemical equation

c)

balanced equation

d)

unbalanced equation

119.

chemical formulas represent

a)

atoms

b)

compounds

c)

elements

d)

balanced equations

120.

NaHCO3 NaBO3 NaClO

a)

chemical formulas

b)

atoms

c)

elements

d)

diatomic molecules

121.

H2 O2

a)

isotopes

b)

atoms

c)

diatomic molecules

d)

isomers

122.

An element symbol with a subscript of 3 indicates

a)

3 atoms of that element are present

b)

the atom has lost 3 electrons

c)

all of these

d)

it is a diatomic molecule

123.

Mg(OH)2

a)

Magnesium Dihydrogen Oxide

b)

Magnesium Hydroxybutyrate

c)

Manganese Hydroxide

d)

Magnesium Hydroxide

124.

C6H12O6

a)

sucrose

b)

glucose

c)

ATP

d)

Amino Acids

125.

H2O2

a)

Water

b)

Hydrogen Peroxide

c)

Dihydrogen Monoxide

d)

Sulfuric Acid

126.

The starting substances on the left in a chemical equation are called

a)

products

b)

reactants

c)

balanced

d)

diatomic molecules

127.

These substances are found on the right side of a chemical equation.

a)

diatomic molecules

b)

reactants

c)

products

d)

balanced equations

128.

What does the arrow in a chemical equation mean?

a)

produces or yields

b)

balanced

c)

sunlight

d)

heat

129.

He discovered that the total mass of the reactants always equals the total mass of the products.

a)

Antoine Lavoisier

b)

Edward Jenner

c)

Jonas Salk

d)

Sir Isaac Newton

130.

The total mass of reactants always equals total mass of products

a)

1st Law of Thermodynamics

b)

Law of Conservation of Energy

c)

Law of Conservation of Mass

d)

2nd Law of Thermodynamics

131.

A number placed in front of an element symbol or chemical formula in an equation.

a)

subscript

b)

coefficient

c)

superscript

d)

exponent

132.

Represents the number of units of a substance

a)

subscript

b)

coefficient

c)

superscript

d)

unbalanced formula

133.

Only this number can be changed when balancing a chemical equation

a)

coefficient

b)

superscript

c)

subscript

d)

exponent

134.

Fe + Cl2 --> FeCl3

a)

unbalanced

b)

balanced

c)

reversible reaction

d)

coefficients are 2 and 3

135.

2Fe + 3Cl2 --> 2FeCl3

a)

unbalanced

b)

balanced

c)

coefficients of 2 and 3

d)

le Chatelier's Principle

136.

The Periodic Table is a chart of the elements arranged into ______ and _________ according to their physical & chemical properties

a)

groups and periods

b)

solid and liquid

c)

solids, liquids and gases

d)

solids and gases

137.

The periodic table has a repeating pattern in boiling point, as you go from left to right which is

a)

lower, then higher, then lower again

b)

lower to higher

c)

higher to lower

d)

higher to lower, then to higher again

138.

these form a "staircase" on the periodic table

a)

nonmetals

b)

metals

c)

metalloids

d)

alkali metals

139.

the majority of elements on the periodic table are found on the left side and are called

a)

metals

b)

nonmetals

c)

lanthanides

d)

noble gases

140.

these have the properties of both metals and nonmetals

a)

metalloids

b)

metals

c)

nonmetals

d)

actinides

141.

Number of natural elements is ____, number of synthetic elements is _____, total number is _______.

a)

92, 25, 117

b)

117, 92, 25

c)

25, 92, 117

d)

34, 17, 146

142.

1. How would you describe, by comparison, the masses of protons, neutrons and electrons?

a)

Electrons have the most mass

b)

Protons have the most mass

c)

Protons and Neutrons have the most mass

d)

Electrons have all the mass

143.

1. Which subatomic particle(s) contain most of an atom’s mass?

a)

Neutrons by a very small margin

b)

Electrons

c)

Protons by a very small margin

d)

Quarks

144.

How many electrons would it take to equal the mass of one proton?

a)

1,840

b)

1

c)

3,000

d)

840

145.

What subatomic particle(s) would you find in the nucleus of an atom?

a)

Protons

b)

Neutrons

c)

Protons & Neutrons

d)

Protons & Electrons

146.

1. What subatomic particle(s) would you find outside the nucleus of an atom?

a)

Electron & Neutron

b)

Electron

c)

Protons

d)

Neutrons

147.

1. What method did Dmetri Mendeleev use to order the first periodic table of elements?

a)

By order of reactivity

b)

By order of ions

c)

By order of atomic mass

d)

By order of atomic number

148.

1. What is an atomic number?

a)

the number of protons and neutrons in an atom

b)

the number of protons in an atom

c)

the number of electrons

d)

the number of extra neutrons

149.

1. What type of electrical charge would you find on Carbon-12?

a)

+1

b)

none

c)

-1

d)

+2

150.

1. Explain why Carbon-13 has no electrical charge.

a)

it has an equal number of protons and neutrons

b)

it has an equal number of electrons and neutrons

c)

It has an equal number of protons & electrons

d)

it has an equal number of protons, neutrons & electrons

151.

What is the difference between Carbon-12 and Carbon-13? What term is used to describe this difference?

a)

They have differing numbers of neutrons & are ions.

b)

They have differing numbers of neutrons & are isomers.

c)

They have differing numbers of neutrons & are isotopes.

d)

They have differing numbers of electrons & are isotopes.

152.

1. What was the most important contribution of Henri Becquerel to the field of Chemistry? What did he discover?

a)

radioactivity, he discovered Uranium

b)

radioactivity, he discovered Polonium

c)

he used a cathode ray tube and discovered the electron

d)

he did the "Gold Foil" experiment & discovered the nucleus

153.

1. Some elements can spontaneously change into other elements. What is the term for this phenomena?

a)

isotopes

b)

radioactivity

c)

ions

d)

covalent bonds

154.

a process that occurs when an unstable atomic nucleus changes into a more stable nucleus

a)

isotope

b)

ion

c)

radioactive decay

d)

covalent bond

155.

three kinds of radioactive decay include :

a)

alpha, beta & omega

b)

beta, gamma & omega

c)

alpha, zeta & gamma

d)

alpha, beta & gamma

156.

this type of radioactive decay turns a neutron into a proton

a)

alpha

b)

beta

c)

gabba

d)

gamma

157.

this type of radioactive particle is made of 2 protons & 2 neutrons

a)

beta

b)

gamma

c)

alpha

d)

gabba

158.

this type of radiation involves high energy levels

a)

alpha

b)

gamma

c)

beta

d)

omega

159.

what is an ion?

a)

an atom with extra or missing electrons

b)

an atom with extra neutrons

c)

an atom with extra protons

d)

at atom that loses protons

160.

this type of ion has extra electrons and has a negative charge

a)

anion

b)

cation

c)

isotope

d)

radioactive

161.

this type of atom is missing electron(s)

a)

isotope

b)

cation

c)

anion

d)

radioactive

162.

this type of atom is missing electron(s)

a)

isotope

b)

cation

c)

anion

d)

radioactive

163.

electrons farthest from the nucleus

a)

have the highest amount of energy

b)

have the lowest amount of energy

c)

can only have 2 electrons

d)

can only have 4 electrons

164.

Atoms can only have this many electrons in their innermost shell

a)

8

b)

2

c)

4

d)

6

165.

chemical properties of an atom are determined by their

a)

ionic properties only

b)

isotopic forms only

c)

innermost electrons

d)

valence shell electrons

166.

Which statement is true?

a)

The number of valence electrons will generally be the different amongst the same group of elements.

b)

The number of valence electrons will generally be the same amongst the same group of elements.

c)

The number of valence electrons will generally be the same amongst the same period of elements.

d)

The number of valence electrons will generally be the same amongst all elements.

167.

Unpaired electrons in an electron dot diagram indicate

a)

where bonds can be formed

b)

nothing

c)

that it is an ion

d)

that it is an isotope

168.

With the exception of ___________, Noble Gases have 8 electrons in their valence shell and are chemically stable.

a)

Helium

b)

Hydrogen

c)

Neon

d)

Bromine

169.

They do not easily react or form bonds with other atoms

a)

halogens

b)

alkali metals

c)

chemically stable atoms

d)

electronegative atoms

170.

What term would you use to describe Neon?

a)

Noble Gas

b)

Chemically Stable

c)

Unreactive

d)

All of these

171.
How many electrons can the 1st electron shell hold?
a)
2
b)
3
c)
8
d)
18
172.
A rule that states that repeating chemical and physical properties of elements change periodically with the atomic number of the elements is the _________.
a)
periodic law
b)
alkaline-earth metals
c)
actinide
d)
group rule
173.
All of the actinides are ___________.
a)
stable
b)
radioactive
c)
shiny
d)
named after scientists
174.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
175.
This class of elements are sometimes called "semiconductors."
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Groups
176.
Why do some elements have 3 letter chemical symbols?
a)
There are no elements with 3 letter symbols
b)
They are named after scientists
c)
They are named after places
d)
They have a temporary name until scientists agree on a new name.
177.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
178.
The yellow atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
179.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
180.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
181.
The periodic table has __ periods.
a)
18
b)
8
c)
2
d)
7
182.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
183.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
184.
What period and group is Silver (Ag)? 
a)
Period 2, Group 1
b)
Period 3, Group 16
c)
Period 5, Group 11
d)
Period 2, 14
185.
The elements in this group have 5 valence electrons and include elements N, P, and As.
a)
Group 5
b)
Group 1
c)
Group 18
d)
Group 15
186.
When chlorine reacts it wants to ______________ electron.
a)
gain 1
b)
lose 1
c)
gain 2
d)
lose 2
187.
Each element wants to gain or lose electrons so that it can have the same electron configuration as......
a)
a Nobel gas
b)
other elements in its family
c)
other elements in its period
d)
it used to have before reacting
188.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon

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