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Quizzziz Hon Unit 1 TEST

Total questions: 175

Worksheet time: 5hrs 18mins

Name
Class
Date
1.
Which of the following are examples of matter?
a)
Dog
b)
Electricity
c)
Air
d)
Ice
2.
Chlorine-37 has how many neutrons?
a)
37
b)
18
c)
20
d)
None of the above
3.
a)
a
b)
b
c)
c
d)
d
4.
The Lanthanide elements are known as the:
a)
Common earth metals
b)
Alkaline earth metals
c)
Rare earth metals
d)
Heavy earth metals
5.
The majority of elements in the periodic table are _____.
a)
Metals
b)
Nonmetals
c)
Metalliods
d)
Gases
6.
Which one of the following atoms has the largest radius?
a)
S
b)
F
c)
Na
d)
Ag
7.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
8.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends.
9.
Francium (Fr) has the lowest ionization energy in Group 1 because -
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus
10.
Which list arranges the elements Na, Li, K, Rb, and Cs in order of increasing ionization energy (from left to right)?
a)
Cs; Rb; K; Na; Li
b)
Cs; Li; Na; K; Rb
c)
Na; Li; K; Rb; Cs
d)
Li; Na; K; Rb; Cs
11.
List the ions from smallest to largest Se2, Zr4+, Mg, Rb+, Br-, K+.
a)
Se2, Zr4+, Mg, Rb+, Br-, K+
b)
Mg, Rb+, Br-, Se2, Zr4+, K+
c)
K+, Br-, Se2, Zr4+, Mg, Rb+,
d)
Zr4+, K+, Rb+, Mg, Br-, Se2
12.
What does an atoms period tell us?
a)
Number of Protons
b)
Number of Valance Electrons
c)
Number of Shells
d)
Number of Neutrons
13.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
Increase, Increase
b)
Decrease, Increase
c)
Decrease, Decrease
d)
Increase, Decrease
14.
In general, as you go across a period in the periodic table from left to right: (1) the atomic radius __________; (2) the electronegativity __________; and (3) the first ionization energy __________.
a)
decreases, decreases, increases
b)
increases, increases, decreases
c)
ncreases, increases, increases
d)
decreases, increases, increases
15.
What does an atoms group/family tell us?
a)
Number of Protons
b)
Number of Valance Electrons
c)
Number of Shells
d)
Number of Neutrons
16.
Which of the following elements would be classified as a metal?
a)
As
b)
Ba
c)
Br
d)
Bo
17.
The family of elements that have one valence electron is the:
a)
noble gas
b)
halogen
c)
alkali metals
d)
isocognogens
18.
The family of elements that is the most unreactive is the :
a)
noble gas
b)
halogen
c)
alkali metals
d)
isocognogens
19.
The elements in this family are soft, silvery, and very reactive with water.
a)
noble gas
b)
halogen
c)
alkali metals
d)
isocognogens
20.
What atom is this?
a)
Boron
b)
Neon
c)
Aluminum
d)
Magnesium
e)
Argon
21.
Which quantum number determines the shape of an orbital?
a)
Principal quantum number (n)
b)
Angular momentum quantum number (l)
c)
Magnetic quantum number (ml)
d)
Spin quantum number (ms)
22.
How many different orbitals are there when l = 3?
a)
3
b)
5
c)
7
d)
9
23.
What element has the following electron configuration? [Ar] 3d104s24p3
a)
As
b)
P
c)
Ga
d)
Se
24.
What are the shapes of the s and p orbitals?
a)
a. s orbitals are spherical and p orbitals are shaped like dumbbells.
b)
b. Both s and p orbitals are spherical.
c)
c. s orbitals are shaped like dumbbells and p orbitals are spherical.
d)
d. s orbitals are spherical and p orbitals are planar.
25.
To move from the ground state to the excited state, an electron:
a)
a. can absorb any amount of energy
b)
b. can release any amount of energy
c)
c. must absorb one or more quanta of energy
d)
d. must release one or more quanta of energy
26.
According to Hund's rule, how does the sixth electron enter the p orbitals in carbon?
a)
It enters the first p orbital with opposite spin as the fifth electron
b)
It enters the second p orbital with opposite spin as the fifth electron
c)
It enters the third p orbital with opposite spin as the fifth electron
d)
It enters the second p orbital with the same spin as the fifth electron
27.
What is the electron configuration of nitrogen?
a)
1s22s22p1
b)
1s22s22p2
c)
1s22s22p3
d)
1s22s22p4
28.
In an electron configuration code, superscripts placed on sub-levels indicate the number of _____.
a)
a. Shells
b)
b. Electrons
c)
c. Sub-shells
d)
d. Orbitals
29.
What is the maximum number of electrons that can occupy an f orbital?
a)
2
b)
4
c)
6
d)
8
30.
What is the ground state of an atom?
a)
The state with the highest energy
b)
The state with the lowest energy
c)
The state with no energy
d)
The state with equal energy levels
31.
How many Valance Electrons will Carbon Have
a)
2
b)
4
c)
6
d)
8
32.
How many electrons are in the 3rd energy level?
a)
2
b)
8
c)
10
d)
18
33.
How many electrons should Boron have around its Lewis dot model?
a)
3
b)
1
c)
2
d)
4
e)
5
34.
Is this the correct Lewis Dot Structure for Boron?
a)
Yes
b)
No, missing electrons
c)
No, too many electrons
d)
No, electrons in wrong place
35.
What atom is shown in the picture?
a)
Sodium (Na)
b)
Fluorine (F)
c)
Sulfur (S)
d)
Potassium (K)
36.
How many orbits will be around Calcium?
a)
4
b)
1
c)
2
d)
3
e)
5
37.
What orbitals can be found in the 3rd energy level?
a)
s
b)
p
c)
d
d)
f
38.
In the symbol pictured what is the number of protons, neutrons and electrons respectively?
a)
12,12,12
b)
12,12,14
c)
12,12,10
d)
12,24,10
39.
How many protons does Lithium Have?
a)
3
b)
1
c)
2
d)
4
e)
5
40.
Calcium has three different isotopes. One has a mass of 35.00 amu; another has a mass of 41.00 amu; and another has a mass of 40.00 amu. Which isotope is the most abundant of the three?
a)
Calcium-35
b)
Calcium-41
c)
Calcium- 40
41.
What Subatomic Particle has a negative charge?
a)
Proton
b)
Electron
c)
Neutron
d)
Quark
42.
What Subatomic Particle has a no charge?
a)
Proton
b)
Electron
c)
Neutron
d)
Quark
43.
The nucleus of an atom contains what 2 parts. Check each one. More that one may be selected
a)
Proton
b)
Neutron
c)
Electron
d)
Lepton
44.
The gold foil experiment proved
a)
existance of electrons
b)
location of electrons
c)
existance of the nucleus
d)
existance of neutrons
45.
The cathode ray experiment proved
a)
existance of electrons
b)
charge of electrons
c)
charge of the neutron
d)
existance of neutrons
46.
What subatomic particle determines the type of atom?
a)
Protons
b)
Electrons
c)
Neutrons
47.
What Charge does an anion have?
a)
Positive
b)
Negitive
c)
No Charge
48.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
49.
Which are intensive properties?
a)
Shape
b)
Mass
c)
Volume
d)
Reactivity
50.
Students are classifying substances. Which of the following is a solution?
a)
Sand and Water
b)
Taco Salad
c)
Water and Oil
d)
Salt and Water
51.
A combination that can be separated by physical processes is a .....
a)
element
b)
compound
c)
mixture
52.
Use the diagram below to answer the following question: Which diagrams represent 3 molecules of a compound?
a)
A
b)
D
c)
I
d)
B
e)
C
53.
A substance that cannot be separated into a simpler substance by chemical or physical means
a)
element
b)
compound
c)
homogenous mixture
d)
hetreogenous mixture
54.
Use the diagram below to answer the following question: Which diagram(s) represent molecules of an element alone?
a)
E
b)
F
c)
A
d)
B
e)
C
55.
What is the charge of the atom in the diagram below?
a)
0
b)
+3
c)
-3
d)
+1
56.
How many protons does Lithium Have?
a)
3
b)
1
c)
2
d)
4
e)
5
57.
Calcium has three different isotopes. One has a mass of 35.00 amu; another has a mass of 41.00 amu; and another has a mass of 40.00 amu. Which isotope is the most abundant of the three?
a)
Calcium-35
b)
Calcium-41
c)
Calcium- 40
58.
What Subatomic Particle has a negative charge?
a)
Proton
b)
Electron
c)
Neutron
d)
Quark
59.
What Subatomic Particle has a no charge?
a)
Proton
b)
Electron
c)
Neutron
d)
Quark
60.
The nucleus of an atom contains what 2 parts. Check each one. More that one may be selected
a)
Proton
b)
Neutron
c)
Electron
d)
Lepton
61.
The gold foil experiment proved
a)
existance of electrons
b)
location of electrons
c)
existance of the nucleus
d)
existance of neutrons
62.
The cathode ray experiment proved
a)
existance of electrons
b)
charge of electrons
c)
charge of the neutron
d)
existance of neutrons
63.
What subatomic particle determines the type of atom?
a)
Protons
b)
Electrons
c)
Neutrons
64.
What Charge does an anion have?
a)
Positive
b)
Negitive
c)
No Charge
65.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
66.
A combination that can be separated by physical processes is a .....
a)
element
b)
compound
c)
mixture
67.
Use the diagram below to answer the following question: Which diagrams represent 3 molecules of a compound?
a)
A
b)
D
c)
I
d)
B
e)
C
68.
a)
a
b)
b
c)
c
d)
d
69.
How many Valance Electrons will Carbon Have
a)
2
b)
4
c)
6
d)
8
70.
How many electrons are in the 3rd energy level?
a)
2
b)
8
c)
10
d)
18
71.
How many electrons should Boron have around its Lewis dot model?
a)
3
b)
1
c)
2
d)
4
e)
5
72.
How many orbits will be around Calcium?
a)
4
b)
1
c)
2
d)
3
e)
5
73.
What orbitals can be found in the 3rd energy level?
a)
s
b)
p
c)
d
d)
f
74.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide?
a)
6
b)
1
c)
2
d)
3
e)
4
75.
Boiling point,melting point, and density are some of an element's ______.
a)
physical properties
b)
chemical properties
76.
A substance that cannot be separated into a simpler substance by chemical or physical means
a)
element
b)
compound
c)
homogenous mixture
d)
hetreogenous mixture
77.
How close a set of measurements are together is called..
a)
accuraccy
b)
precision
c)
estimation
d)
significance
78.
How close a measurement is to the accepted value is called..
a)
accuraccy
b)
precision
c)
estimation
d)
significance
79.
Which set of properties, intensive or extensive, are based on the size of a sample?
a)
intensive
b)
extensive
80.
Four students obtained the following measurements, seen below, using a ruler while measuring a piece of metal ribbon. The actual length, as recorded by the teacher, was 30.5 cm. Each student measured the metal ribbon 4 times using the same ruler each time. Which of the following statements regarding the four students’ measurements are correct?
a)
Ramshi’s measurements were both accurate and precisetion 1
b)
Ai’s measurements were accurate and precise
c)
Becky’s measurements were accurate; but not precise
d)
Kara’s measurements were precise but not accurate
81.
What is the purpose of scientific notation?
a)
to measure things
b)
to represent very large or very small numbers
c)
to complicate things
d)
Both A&B
82.
A solution is considered to be a _____.
a)
homeogenous mixture
b)
hetreogenous mixture
c)
pure substance
83.

Which term refers to two or more substances that are blended but are not chemically bonded?

a)

compound

b)

element

c)

mixture

d)

molecule

84.

What do we call a substance that consists of only one type of atom?

a)

Atom

b)

Element

c)

Compound

d)

Substance

85.

A mixture in which two or more substances are evenly mixed but are not bonded togather is?

a)

A homogeneous mixture.

b)

A heterogeneous mixture.

c)

A mixture.

d)

A solution.

86.

Which term refers to the region surrounding an atoms nucleus where one or more electrons are most likely to be found?

a)

electron cloud

b)

ion

c)

isotope

d)

proton

87.

Which term describes one of two or more atoms of an element having the same number of protons, but a different number of neutrons?

a)

atomic number

b)

ion

c)

isotope

d)

molecule

88.

Which describes the region at the centre of an atom that contains most of the mass of the atom?

a)

proton

b)

nucleus

c)

neutron

d)

electron

89.

Which of the following defines matter?

a)

Anything that has mass and takes up space.

b)

Anything that has density.

c)

Mass over volume.

d)

It doesn't matter.

90.

An element's atomic number gives us which of the following:

a)

Protons and neutrons

b)

Neutrons and electrons

c)

Protons and electrons

d)

Number of orbitals

91.

The mass number of an element gives us which of the following:

a)

Protons + Neutrons

b)

Protons + Electrons

c)

Electrons + Neutrons

d)

Jimmy + Neutron

92.

What is the BEST way to find the number of neutrons in an atom?

a)

Look at the atomic structure

b)

It is the same as the number of electrons

c)

Subtract the atomic number from the mass number

d)

Neutrons are not real

93.

Chlorine has an atomic number of 17 and has 18 neutrons. What is it mass number?

a)

35

b)

18

c)

17

d)

1

94.
The the smallest particle of an element that still has the element’s properties.
a)
proton
b)
neutron
c)
atom
d)
electron
95.
Pure substances—such as nickel, hydrogen, and helium—that make up all kinds of matter.
a)
element
b)
atom
c)
proton
d)
neutron
96.
These have a positive electric charge and are found in the nucleus of an atom.
a)
electron
b)
neutron
c)
proton
97.
These have a negative electric charge and move around outside the nucleus.
a)
electron
b)
proton
c)
neutron
98.
These are neutral in electric charge and are  found in the nucleus.
a)
electron
b)
proton
c)
neutron
99.
___ is a measure of the amount of matter in a substance or an object.
a)
Volume
b)
Density
c)
Mass
100.
This law states that matter cannot be created or destroyed.
a)
Law of Superposition
b)
Law of Gravity
c)
Law of Conservation of Mass
d)
Law of Stratigraphy
101.
Pure substances made up of only one type of atom that cannot be broken down into a simpler substance.
a)
Compounds
b)
Protons
c)
Nucleus
d)
Elements
102.
A substance formed by more than one type of atom.
a)
Compound
b)
Element
c)
Gas
d)
Molecule
103.
An organized table of all the elements (pure substances).
a)
Periodic Table 
b)
Atoms
c)
Compounds
d)
Molecules
104.

A solid turning into a liquid is:

a)

Vaporation

b)

Freezing

c)

Melting

d)

Deposition

e)

Sublimation

105.

A liquid turning into a solid is:

a)

Freezing

b)

Melting

c)

Condensation

d)

Sublimation

106.

A solid turning into a gas is:

a)

Melting

b)

Sublimation

c)

Condensation

d)

Deposition

107.

How many protons does this atom have?

a)

4

b)

5

c)

9

d)

13

108.

How many electrons are in the nucleus of this atom?

a)

0

b)

3

c)

6

d)

7

e)

4

109.
What are the three states of matter?
a)
solid, volume, mass
b)
density, volume, mass
c)
solid, liquid, gas
d)
density, gas, volume
110.
Gasoline is a ________________.
a)
liquid
b)
solid
c)
gas
111.
Sand is a ___________________.
a)
liquid
b)
solid
c)
gas
112.

What type of mixture is air (with smog) ?

a)

Homogeneous

b)

Heterogeneous

113.

What type of mixture is chocolate chip ice cream?

a)

Homogeneous

b)

Heterogeneous

114.

Which of the following are pure substances?

a)

Carbon dioxide (CO2)

b)

Milk

c)

Salt water

d)

Nitrogen (N2)

115.

Which of the following are mixtures?

a)

Sodium bicarbonate (NaHCO3)

b)

Steel (Fe + C)

c)

Salt water (NaCl + H2O)

d)

Gold (Au)

116.

Which of the following are evidences or a chemical change?

a)

Change of color (unintended)

b)

Change of shape

c)

Change of size

d)

Change of odor

117.

What is the main evidence that a chemical change has occured?

a)

Change of color

b)

Production of Bubbles

c)

Production of Fire

d)

A new substance is produced

118.

Which of the following are evidences of a physical change?

a)

Change of size

b)

Change of color

c)

Change of state of matter

d)

Change of odor

119.

What is the classification of physical properties?

a)

Uniform / Non uniform

b)

Intensive / Extensive

c)

Independent / Dependent

d)

There is no classification

120.

Which of the following are examples of intensive properties?

a)

Conductivity

b)

Mass

c)

Length

d)

Density

121.

Which of the following are examples of chemical properties?

a)

Conductivity

b)

Flammability

c)

Reactivity

d)

Malleability

122.

Which of the following are examples of chemical changes?

a)

Burning paper

b)

Cutting paper

c)

Iron rusting

d)

Wrinking paper

123.

Which of the following are physical changes?

a)

Cutting your hair

b)

Fruit rotting

c)

Water boiling

d)

Dropping an alka-seltzer in water

124.

Which of the following are extensive properties?

a)

Mass

b)

Volume

c)

Density

d)

Temperature

125.
Which of the following tells you that a chemical change may have occurred?
a)
Change Shape
b)
Melting
c)
Vaporizing
d)
Change in color
126.
What happens in ALL chemical changes?
a)
Change in state of matter
b)
A new substance is formed
c)
Bubbles are produced
d)
An explosion
127.
Is wood burning a physical or chemical change?
a)
Physical 
b)
Chemical
128.
Is milk going sour a physical or chemical change?
a)
Physical 
b)
Chemical
129.
Is Gatorade powder dissolving in water physical or chemical change?
a)
Physical 
b)
Chemical
130.
Is mold growing on cheese a physical or chemical change?
a)
Physical 
b)
Chemical
131.
Is making orange juice a physical or chemical change?
a)
Physical 
b)
Chemical
132.
Is sharpening a pencil a physical or chemical change?
a)
Physical 
b)
Chemical
133.
Is copper tarnishing a physical or chemical change?
a)
Physical 
b)
Chemical
134.
The Law of Conservation of Mass tells us matter can't  ______________.
a)
change color
b)
change state of matter
c)
be created or destroyed
d)
change temperature
135.
Which of the following IS a clue that a chemical change has occurred? 
a)
State of matter change
b)
Size Change
c)
Change in temperature
d)
Shape change
136.

Which one of the following discoveries came first?

a)

electrons

b)

neutrons

c)

quarks

d)

atoms

137.

Rutherford and his students did experiments that showed

a)

quark

b)

nucleus

c)

proton

d)

electron

138.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

139.

Which scientist discovered that the nucleus contained neutrons?

a)

bohr

b)

Rutherford

c)

Dalton

d)

Chadwick

140.

What is a particle with one negative charge called?

a)

electron

b)

proton

c)

quark

d)

neutron

141.

The smallest particle of an element that still represents that element.

a)

Nucleus

b)

electron

c)

proton

d)

atom

142.

What is a particle with one positive charge called?

a)

proton

b)

electron

c)

neutron

d)

quark

143.

What is the neutral particle found in the nucleus called?

a)

proton

b)

neutron

c)

electron

d)

quark

144.

What is the center of an atom called?

a)

nucleus

b)

electron cloud

c)

proton center

d)

photon center

145.

Which one of the following parts of the atom is the smallest?

a)

atom

b)

neutron

c)

quark

146.

Which one of the following parts of the atom is the smallest?

a)

electron cloud

b)

electron

c)

nucleus

147.

Which one of the following is the correct order of scientific contribution of the atom?

a)

Chadwick, Dalton, Bohr, Rutherford, Democritus,Thomson

b)

Thomson, Democritus,Rutherford, Bohr, Dalton ,Chadwick

c)

Dalton, Chadwick ,Bohr, Rutherford, Democritus,Thomson

d)

Democritus, Dalton, Thomson, Rutherford, Bohr, Chadwick

148.
Who discovered that the nucleus contains positively charged particles called protons?
a)
Ernest Rutherford
b)
James Chadwick
c)
Democritus
d)
Niels Bohr
149.
all matter is made of what 
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
150.
In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.
a)
Atoms
b)
Parts
c)
Molecules
d)
Hydrogen
151.
Which model is this?
a)
Thomson Model
b)
Cloud Model
c)
Bohr Model
d)
Rutherford Model
152.
Which model involved gold foil?
a)
Thomson Model
b)
Rutherford Model
c)
Cloud Model
d)
Bohr Model
153.
Which of these particles was discovered first?
a)
Protons
b)
Electrons
c)
Neutrons
d)
Quarks
154.

Who was the Greek philosopher who called the smallest particle of matter as "atom"?

a)

Democritus

b)

Aristotle

c)

J.J Thompson

d)

Einstein

155.
Who is the scientist who proposed the "solar system" model of an atom where the electrons revolve around the nucleus?
a)
Dalton
b)
Niels Bohr
c)
Ernest Rutherford
d)
Democritus
156.
What did James Chadwick discover?
a)
neutrons
b)
electrons
c)
the atomic theory
d)
protons
157.
Which scientist developed the plum pudding/chocolate chip cookie model
a)
Dalton
b)
Thompson 
c)
Rutherford
d)
Democritus
158.
Which scientist saw the atom as a solid sphere?
a)
Dalton
b)
Thomson
c)
Rutherford
d)
Bohr
159.

Which of the following is/are conclusions based on Rutherford’s gold foil experiment?

a)

Atom is mostly empty space

b)

The nucleus is positively charged

c)

The atom has a small dense nucleus

d)

All answers are correct

160.

Developed an atomic theory of matter.

a)

Chadwick

b)

Millikan

c)

Rutherford

d)

Dalton

161.

Used cathode rays to experiment with atoms.

a)

Rutherford

b)

Dalton

c)

Thomson

d)

Millikan

162.

Used alpha particles to discover the nucleus

a)

Thomsan

b)

Becquerel

c)

Millikan

d)

Rutherford

163.
Who stated that all atoms of the same element are excacty alike?
a)
Democritus
b)
Dalton
c)
Thomson
d)
Borh
164.
These particles orbit around the nucleus of an atom.  What are they called?
a)
electrons
b)
protons
c)
neutrons
d)
photons
165.
What is the atomic number of this nucleus?
a)
1
b)
3
c)
4
d)
7
166.

Who is accredited for naming the atom?

a)

Dalton

b)

Thomson

c)

Democritus

d)

Bohr

167.
Which experiment was performed by J. J. Thompson in 1897?
a)
Oil Drop Experiment
b)
Gold Foil Experiment
c)
Wave  Experiment
d)
Cathode Ray Experiment
168.
Who performed the Gold Foil Experiment?
a)
J. J. Thomson
b)
Ernest Rutherford
c)
Neils Bohr
d)
John Dalton
169.
Which model was proposed by Neils Bohr?
a)
Planetary Model
b)
Plum Pudding Model
c)
Quantum Mechanical Model
d)
Solid Ball Model
170.
Which scientist disagreed with the idea that atoms existed?
a)
Democritus
b)
Aristotle
c)
Rutherford
171.
He believed that all matter was continuous and that four basic elements existed (earth, wind, fire, water).
a)
Democritus
b)
Aristotle
c)
Chadwick
d)
Thomson
172.

Which scientist was the first to benefit from the Lavoisier's efforts to define pure substances in the 1700's?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

173.
Determined that electron paths cannot be predicted and exist inside the Electron Cloud.
a)
Schrodinger & Heisenberg
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
174.
How many protons does an atom with an atomic number of 28 and a mass number of 40 have?
a)
28
b)
68
c)
12
d)
40
175.
The following element has _____________ electrons.
a)
114
b)
289
c)
175
d)
403