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3rd NIne Weeks Studyguide

Total questions: 131

Worksheet time: 3hrs 32mins

Name
Class
Date
1.
What type of particles exist within an atomic nucleus?
a)
Protons and Neutrons
b)
Neutrons and electrons
c)
Neutrons and Atoms
d)
Elements and Atoms
2.
Oxygen has an atomic number of 8. What can you conclude?
a)
An atom of oxygen weighs 8 atoms
b)
An atom of oxygen has 4 protons and 4 electrons
c)
An atoms of oxygen has 8 postitrons
d)
An atom of oxygen has 8 protons
3.

What is the mass number of the most common isotope of Fluorine?

a)

18.9984

b)

9

c)

18

d)

19

4.

Who started the modern atomic theory (backed with data) of the atom?

a)

Democritus

b)

Dalton

c)

Thomson

d)

Bohr

5.
All atoms of the same element have the same?
a)
number of neutrons
b)
number of protons
c)
mass number
d)
all of these
6.

What is the mass number of an atom of hydrogen that has 1 neutron?

a)

0

b)

1

c)

2

d)

3

7.

Elements are made of tiny solid particles

a)

Bohr

b)

Democritus

c)

Thomson

d)

Aristole

8.

All matter is made of atoms

a)

Rutherford

b)

Bohr

c)

Democritus

d)

Dalton

9.

Most mass in an atom is in the nucleus

a)

Rutherford

b)

Thomson

c)

Bohr

d)

Dalton

10.

electrons travel in fixed orbits

a)

Dalton

b)

Bohr

c)

Thomson

d)

Rutherford

11.

"Atomos" atoms always move

a)

Bohr

b)

Democritus

c)

Julius Cesar

d)

Heisenberg

12.

Who believed that atoms are small solid objects that cannot be divided, created, or destroyed?

This person also believed atoms are constantly moving in empty space.

a)

Democritus

b)

John Dalton

c)

J.J. Thomson

d)

Ernest Rutherford

13.

Who discovered the existence of electrons and did NOT believe that atoms were a single solid object?

a)

Democritus

b)

John Dalton

c)

J.J. Thomson

d)

Ernest Rutherford

14.

Who believed that all matter is made of atoms that cannot be divided, created, or destroyed, and during a chemical reaction, atoms of one element cannot be converted into atoms of another element?

a)

Democritus

b)

John Dalton

c)

J.J. Thomson

d)

Ernest Rutherford

15.

Who believed that atoms are made mostly of empty space, and most of an atom's mass and positive charge is concentrated in a small area in the center of an atom called the nucleus?

a)

Democritus

b)

John Dalton

c)

J.J. Thomson

d)

Ernest Rutherford

16.

Who believed that different types of matter are made of different types of atoms and the properties of the atoms determine the properties of the matter?

a)

Democritus

b)

John Dalton

c)

J.J. Thomson

d)

Ernest Rutherford

17.

Who believed that atoms were an evenly distributed positive charge with negative charges mixed randomly throughout?

a)

Democritus

b)

John Dalton

c)

J.J. Thomson

d)

Ernest Rutherford

18.

Who believed that atoms of one element are identical to each other but different from atoms of another element? This person also believed that atoms combine in specific ratios.

a)

Democritus

b)

John Dalton

c)

J.J. Thomson

d)

Ernest Rutherford

19.

Who believed that negatively charged particles (electrons) move in the empty space surrounding the nucleus?

a)

Democritus

b)

John Dalton

c)

J.J. Thomson

d)

Ernest Rutherford

20.

Who believed that electrons orbit the nucleus in different energy levels and the closer to the nucleus the electron is, the less energy it has?

a)

James Chadwick

b)

John Dalton

c)

Niels Bohr

d)

Ernest Rutherford

21.

Who believed that in addition to protons, the nucleus of an atom contains neutrally charged particles called neutrons?

a)

James Chadwick

b)

John Dalton

c)

Niels Bohr

d)

Ernest Rutherford

22.

Who believed that when an electron moves to a lower energy level, a specific amount of energy is released?

a)

James Chadwick

b)

John Dalton

c)

Niels Bohr

d)

Ernest Rutherford

23.
a)
Periods
b)
Groups
24.
a)
Periods
b)
Groups
25.

Today, the elements on the periodic table are arranged_____.

a)

atomic number (top number)

b)

atomic mass (bottom number)

c)

alphabetically

26.

These elements are in a:

a)

group

b)

period

27.
What is the Atomic Symbol?
a)
MG
b)
Mg
c)
Ma
d)
P
28.
What is the Atomic Number
a)
12
b)
24
c)
24.305
d)
48
29.
What is the Atomic Mass?
a)
12
b)
24
c)
24.305
d)
48
30.

What Group is Magnesium in?

a)

3

b)

2

c)

4

d)

5

31.
What Period is Magnesium in?
a)
3
b)
2A
c)
4
d)
3A
32.

The period for Bromine is ___________.

a)

3

b)

2

c)

4

d)

5

33.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
34.

The atomic number is the same as the:

a)

electrons

b)

neutrons

c)

protons

d)

atomic mass

35.

Look at the image. What is the atomic number for carbon?

a)

12.011

b)

6

c)

7

d)

8

36.

Look at the image. How many protons does carbon have?

a)

12.011

b)

6

c)

4

d)

5

37.

Look at the image. What is the atomic number for oxygen?

a)

15.999

b)

16

c)

8

d)

9

38.
What is the mass number defined as?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
39.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

40.

What is the mass number and atomic number ?

a)

Mass number = 7, atomic number = 14

b)

Mass number = 14, atomic number = 7

41.

Which subatomic particle has a negative charge in the atom?

a)

proton

b)

neutron

c)

electron

d)

quark

42.

The chemical symbol for nitrogen.

a)

N

b)

Cl

c)

Fe

d)

Pb

43.

The chemical symbol for chlorine.

a)

C

b)

Cl

c)

Fe

d)

Pb

44.

The chemical symbol for sodium.

a)

C

b)

H

c)

O

d)

Na

45.

The chemical symbol for hydrogen.

a)

C

b)

H

c)

O

d)

Na

46.

The chemical symbol for oxygen.

a)

C

b)

H

c)

O

d)

Na

47.

The chemical symbol for carbon

a)

C

b)

H

c)

O

d)

Na

48.
Which of the following best describes an atom?
a)
protons and neutrons grouped together
b)
protons and electrons grouped together
c)
a core (center) of protons and neutrons surrounded by electrons
d)
a core of electrons and neutrons surrounded by protons
49.

Which of the following is correct for a neutral atom ?

a)

the number of protons and neutrons are the same

b)

the number of protons and electrons are the same

c)

the number of electrons and neutrons are the same

d)

the atomic and mass numbers are the same

50.

The number of protons and neutrons in an atomic is called it's :

a)

atomic number

b)

mass number

c)

oxidation number

d)

phone number

51.

Atoms of the same element with different mass numbers have a different number of :

a)

protons

b)

neutrons

c)

electrons

d)

mesons

52.
What makes an atom have a positive charge?
a)
more electrons than protons
b)
more neutrons than electrons
c)
more protons than electrons
d)
less protons than electrons
53.

Cobalt (Co) has 27 protons in each atom. Based on this information, which of the following also describes an atom of Cobalt? assuming the atom is neutral

a)

It has no neutrons.

b)

It has 27 electrons.

c)

It has 13 neutrons and 14 electrons.

d)

It has a total of 86 neutrons and electrons.

54.
Iodine (I) has 53 electrons in each atom. Based on this information, which of the following also describes an atom of silver?
a)
It has 53 neutrons.
b)
It has 53 protons.
c)
It has 27 neutrons and 26 electrons.
d)
It has a total of 180 neutrons and electrons.
55.
An element with an atomic number of 37 and an atomic mass of 85 has how many neutrons in each atom?
a)
37
b)
48
c)
85
d)
122
56.
An atom has 54 protons, 54 electrons, and 131 neutrons. What is the atomic number of the atom?
a)
54
b)
77
c)
131
d)
185
57.

Atom atom of Carbon has an atomic number of 6 and a mass number of 14. Which of the following is correct ?

a)

it has 6 protons, 8 electrons and 8 neutrons

b)

It has 8 protons, 6 electrons and 6 neutrons

c)

It has 8 protons, 8 electrons and 6 neutrons

d)

It has 6 protons, 6 electrons and 8 neutrons

58.

Which subatomic particle has a positive charge?

a)

proton

b)

neutron

c)

electron

d)

midichlorian

59.

Which subatomic particle has a negative charge?

a)

proton

b)

neutron

c)

electron

d)

cybertron

60.

What is the center of an atom called?

a)

The headquarters

b)

The centrometer

c)

The hypothesis

d)

The nucleus

61.

The nucleus of an atom contains which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, electrons, and neutrons

62.

Typically in an atom, which two subatomic particles are equal in number?

a)

protons and neutrons

b)

all subatomic particles are equal in number

c)

neutrons and electrons

d)

protons and electrons

63.

What is the atomic mass of Neon?

a)

10

b)

20.18

c)

10.18

d)

30.18

64.

How many electrons does an atom of Krypton have?

a)

36

b)

83.80

c)

48

d)

119.80

65.

If an atom has six positively charged subatomic particles, which of the following must it also have in order to become a neutral atom?

a)

Twelve protons

b)

Six neutrons

c)

Three electrons

d)

Six electrons

66.

A neutral atom has an equal number of positive and negative charges. If a neutral fluorine atom has 9 protons and 10 neutrons, how many electrons will it have?

a)

10

b)

9

c)

8

d)

7

67.

What is the name for the type of subatomic particle that is electrically neutral and found in the nucleus of an atom?

a)

Proton

b)

Neutron

c)

Ion

d)

Electron

68.

Which subatomic particles(s) would be found orbiting around the nucleus?

a)

Electrons and protons

b)

Neutrons only

c)

Protons and neutrons

d)

Electrons only

69.

Which subatomic particle has a positive charge?

a)

proton

b)

neutron

c)

electron

d)

midichlorian

70.

Which subatomic particle has a negative charge?

a)

proton

b)

neutron

c)

electron

d)

cybertron

71.
How many electrons does an atom of Krypton have?
a)
36
b)
83.80
c)
47.80
d)
119.80
72.
The subatomic particle that is located in the nucleus of an atom with a neutral charge...
a)
Proton
b)
Neutron
c)
Electron
d)
Quark
73.
How many neutrons does Argon have in it's nucleus?
a)
39.948
b)
58
c)
22
d)
18
74.
How many protons are in Cadmium?
a)
112.411
b)
170
c)
64
d)
48
75.
The ______________ is the number of protons + neutrons in the nucleus of an atom.
a)
atomic number
b)
net charge
c)
chemical symbol
d)
atomic mass
76.
Calculate the atomic number of an atom with :
2 protons
3 neutrons
4 electrons
a)
2
b)
3
c)
4
d)
5
77.
Calculate the atomic weight/mass of an atom with:
11 protons
10 neutrons
11 electrons
a)
11
b)
21
c)
22
d)
10
78.

Number of protons - number of electrons = charge of an atom

a)

True

b)

False

79.

To calculate the number of protons, neutrons, and electrons in an atom, use the atomic number (which equals the number of protons) and the mass number (sum of protons and neutrons).

a)

True

b)

False

80.

________ always equal the atomic number of an element.

a)

Proton

b)

Electron

c)

Neutron

81.

In a neutral atom, equal to the atomic number (same as the number of protons)

a)

Proton

b)

Electron

c)

Neutron

82.

Calculated my subtracting atomic number from the mass number.

a)

Proton

b)

Electron

c)

Neutron

83.

The average mass of an element's isotopes, weighted according to how common each isotope is.

a)

Atomic number

b)

Mass Number

c)

Average Atomic Mass

84.

A substance made from one type of atom. It cannot be changed into anything simpler

a)

element

b)

compound

c)

mixture

85.

This substance represents....

a)

an atom

b)

a compound

c)

a mixture

d)

a molecule

86.
DIFFERENT kinds of atoms chemically combined to form a substance are
a)
Mixture
b)
Element
c)
Compound
d)
Substance
87.
This contains a variety elements and compounds that ARE NOT chemically combined.
a)
Water
b)
Mixture
c)
Elements
d)
Compounds
88.
A pure substance...
a)
is an element or a compound
b)
is an element or a mixture
c)
is a compound or a mixture
d)
is a mixture
89.

A pure substance made of one or more elements.

a)

substance

b)

atom

c)

compound

d)

element

90.

How do elements differ from other pure substances?

a)

Elements and Pure Substances are the same.

b)

Pure substance cannot be broken down into substances.

c)

Elements can be broken down into substances.

d)

Elements can NOT be broken down into substances.

91.

A substance that is composed of just one type of matter.

a)

element

b)

compound

c)

mixture

92.

Matter that can vary in its composition and is made up of two or more substances. Substances in a a _____ do not combine chemically.

a)

element

b)

compound

c)

mixture

93.

A type of substance containing two or more elements that are bonded together. Ex: Water

a)

element

b)

compound

c)

mixture

94.

____ a type of mixture where the particles are non-uniform and unevenly distributed.

a)

homogenous

b)

heterozygous

c)

homozygous

d)

heterogeneous

95.

____ is a type of mixture where you can see the particles

a)

homogeneous

b)

heterogeneos

c)

homozygous

d)

heterozygous

96.

____ is a mixture where particles are uniform and evenly distributed.

a)

homogenous

b)

heterogeneous

c)

heterozygous

d)

homozygous

97.

Properties that can only be observed or measured by changing the chemical identity of a substance.

a)

Physical Properties

b)

Combustible Properties

c)

Chemical Properties

d)

Changeable Properties

98.

When a new substance is formed with different properties than the original substance it is called a...

a)

Chemical change

b)

Physical change

c)

Change in State

d)

Change in appearance only.

99.

elements

a)

each of more than one hundred substances that cannot be chemically interconverted or broken down into simpler substances and are primary constituents of matter. Each element is distinguished by its atomic number, i.e. the number of protons in the nuclei of its atoms.

b)

a part or aspect of something abstract, especially one that is essential or characteristic:

c)

the rudiments of a branch of knowledge:

d)

a group of people of a particular kind within a larger group or organization:

100.

compound

a)

a thing that is composed of two or more separate elements; a mixture:

b)

made up or consisting of two or more existing parts or elements

c)

make (something bad) worse; intensify the negative aspects of

d)

make up (a composite whole); constitute:

101.

Mixtures

a)

a substance made by mixing other substances together:

b)

the process of mixing or being mixed.

c)

a combination of different qualities, things, or emotions in which the component elements are individually distinct:

d)

a person regarded as a combination of qualities and attributes:

102.

what are examples of elements

a)

helium, iron, and neon

b)

hydrogen and oxygen

103.

what are examples of a compound

a)

any substance with more than one element and a fixed ratio between them

b)

  • Water. Chemical Formula: H₂O. Composition: 2 hydrogen atoms, 1 oxygen atom.

  • Sodium Chloride (Table Salt) Chemical Formula: NaCl. Composition: 1 sodium atom, 1 chlorine atom.

  • Carbon Dioxide. Chemical Formula: CO₂ Composition: 1 carbon atom, 2 oxygen atoms.

  • Glucose. Chemical Formula: C₆H₁₂O₆ Composition: 6 carbon atoms, 12 hydrogen atoms,

c)

all of the above

104.

what are examples of mixtures

a)

Oil and water. Lemon juice and tea. Honey and tea. Milk and chocolate. Coffee and cream. Cream and sugar. Flour and butter. Cereal and milk.

b)

homogeneous and heterogeneous

105.

what are the types of mixtures of elements

a)

homogeneous mixtures and heterogeneous mixtures

b)

your mom

106.

what are the types of mixtures of compounds

a)
Liquid and solid mixtures
b)
Homogeneous mixtures and heterogeneous mixtures
107.

what are the types of mixtures

a)
Colloidal mixtures
b)
Homogeneous mixtures and heterogeneous mixtures
108.

solvent definition

a)
A solvent is a substance that dissolves a solute.
b)
A solvent is a substance that cannot dissolve anything.
109.

solute definition

a)
A solute is a type of solvent.
b)
A solute is a mixture of two or more substances.
c)
A solute is a substance that cannot be dissolved.
d)
A solute is a substance that is dissolved in a solvent.
110.

solution definition

a)
response
b)
solution
c)
answer
d)
conclusion
111.

solvent examples

a)
Olive oil, glycerin, propane
b)
Water, ethanol, acetone, benzene
c)
Ammonia, bleach, mercury
d)
Salt, sugar, vinegar
112.

solute examples

a)
Oxygen
b)
Hydrogen
c)
Nitrogen
d)
Salt, sugar, carbon dioxide
113.

solution examples

a)
solution definitions
b)
solution illustrations
c)
solution examples
d)
solution descriptions
114.

what is solids changes in state

a)
Solids change state only through freezing.
b)
Solids can only change state by dissolving in liquids.
c)
Solids do not change state under any conditions.
d)
Solids change state primarily through melting and sublimation.
115.

what is liquids changes in state

a)
Sublimation, precipitation, and filtration
b)
Condensation, precipitation, and solidification
c)
Melting, boiling, and crystallization
d)
The changes in state of liquids include evaporation, condensation, freezing, and melting.
116.

what is gas changes of matter

a)
Gas is always a solid at room temperature.
b)
Gas is a state of matter that can change to liquid or solid through processes like condensation and freezing.
c)
Gas cannot change to any other state of matter.
d)
Gas is a liquid that evaporates into vapor.
117.

what is plasma changes in state

a)
Plasma changes state through ionization and recombination.
b)
Plasma changes state via sublimation and deposition.
c)
Plasma changes state by freezing and melting.
d)
Plasma changes state through condensation and evaporation.
118.

solids examples

a)
water
b)
Metals, wood, ice, rocks
c)
air
d)
sand
119.

liquids examples

a)
Water, milk, oil
b)
Glass, metal, wood
c)
Air, fire, earth
d)
Sand, sugar, salt
120.

gas examples

a)
Oxygen, nitrogen, carbon dioxide, helium
b)
Methane
c)
Ammonia
d)
Water vapor
121.

plasma examples

a)
Water, ice, steam
b)
Stars, lightning, neon signs
c)
Carbon dioxide, oxygen, nitrogen
d)
Wood, metal, glass
122.

physical properties

a)
Physical properties are only related to temperature.
b)
Physical properties cannot be measured directly.
c)
Physical properties are subjective interpretations of matter.
d)
Physical properties are observable characteristics of matter.
123.

chemical properties

a)
Chemical properties describe the color and texture of a substance.
b)
Chemical properties are characteristics that describe how a substance interacts with other substances during a chemical reaction.
c)
Chemical properties are only related to physical changes.
d)
Chemical properties are irrelevant in chemical reactions.
124.

changes

a)
Corrections or fixes.
b)
Revisions or updates.
c)
Improvements or enhancements.
d)
Modifications or alterations.
125.

physical properties examples

a)
Examples of physical properties include color, density, melting point, boiling point, and solubility.
b)
magnetism
c)
taste
d)
hardness

126.

Answer the questions below after watching the video

126.

chemical properties example

a)
Solubility in water
b)
Color change upon heating
c)
Density measurements
d)
Reactivity with acids, flammability, oxidation states.

127.

Answer the questions below after watching the video

127.

changes example

a)
Changing the value of a variable from 0 to 5.
b)
Changing the value of a variable from 5 to 15.
c)
Changing the value of a variable from 10 to 5.
d)
Changing the value of a variable from 5 to 10.
128.

what is the formula for density

a)
Density = Volume / Mass
b)
Density = Mass + Volume
c)
Density = Mass x Volume
d)
Density = Mass / Volume
129.

what is the formula for pressure

a)
Pressure = Force / Area
b)
Pressure = Force + Area
c)
Pressure = Area / Force
d)
Pressure = Mass / Volume
130.

calculate pressure

a)
P = A/F
b)
P = F - A
c)
P = F/A
d)
P = F + A

131.

Answer the questions below after watching the video

131.

calculate density

a)
Density = Mass / Volume
b)
Density = Mass x Volume
c)
Density = Mass + Volume
d)
Density = Volume / Mass

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