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C1 up to periodic table

Total questions: 59

Worksheet time: 53mins

Name
Class
Date
1.

What is the smallest unit of matter? It is composed of protons and neutrons, held together in the nucleus, and electrons around the nucleus in different electron orbitals, which form an electron cloud.

a)

cell

b)

nucleus

c)

atom

d)

electron

2.

What are any of the various self-contained units of matter or energy that are fundamental parts of all matter. These particles include electrons, protons, and neutrons.

a)

subatomic particles

b)

elements

c)

nucleus

d)

electron cloud

3.

What is a subatomic particle with a positive charge that is in the nucleus of an atom?

a)

neutron

b)

proton

c)

electron

d)

valence electron

4.

What is a subatomic particle without an electric charge, located in the nucleus of an atom?

a)

neutron

b)

proton

c)

electron

d)

valence electron

5.

What is a subatomic particle with a negative charge? It is found in the electron cloud surrounding the nucleus.

a)

neutron

b)

proton

c)

electron

d)

electron cloud

6.

What is the system of electrons surrounding the nucleus of an atom?

a)

valence electrons

b)

nucleus

c)

electrons

d)

electron cloud

7.

What is the center of an atom containing protons and neutrons?

a)

nucleus

b)

neutron

c)

proton

d)

electron cloud

8.

What is the number of protons in the nucleus of an atom that determines the chemical properties of an atom?

a)

mass number

b)

atomic mass

c)

atomic number

d)

atomic symbol

9.

What is the combined mass of all the protons and neutrons of an atom and is approximately equal to the number of protons and neutrons?

a)

atomic mass

b)

atomic number

c)

subatomic particles

d)

nucleus weight

10.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons in the energy levels

11.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

12.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

13.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

14.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of e- and p+ together
b)
Subtract the number of e- from p+
c)
Subtract the number of p+ from the mass number
d)
Add the mass number to the number of e-
15.
If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?
a)
12 neutrons
b)
12 electrons
c)
12 protons
d)
24 protons and neutrons
16.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

17.

How many electrons does this atom have?

a)

2

b)

4

c)

6

d)

10

18.
What is the atomic number of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
19.

Is the number below the element symbol on the periodic table the mass number?

a)

Yes!

b)

NO!!

20.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
21.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
22.

What is the charge of a sodium ion?

a)

+2

b)

+1

c)

-1

d)

-2

23.
What charge will an Oxygen ion have? 
a)
+1
b)
-1
c)
+2
d)
-2
24.
charge of beryllium ion
a)
-2
b)
-1
c)
+1
d)
+2
25.
charge of lithium ion
a)
-2
b)
-1
c)
+1
d)
+2
26.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
27.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
28.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
29.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
30.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
31.
A Silicon atom wants...
a)
3 more electrons
b)
3 less electrons
c)
4 more or less electrons
d)
2 more electrons
32.
A Radium atom wants...
a)
One more electron
b)
One less electron
c)
Two more electrons
d)
Two less electrons
33.
What is an isotope? 
a)
A charged atom
b)
An atom with different amounts of neutrons
c)
An atom with different amounts of protons
d)
A neutral atom
34.
The photo above shows the isotopic notation for which isotope?
a)
Carbon 12
b)
Carbon 13
c)
Carbon 14
d)
Carbon 15
35.
Different isotopes have...
a)
different masses
b)
different atomic numbers
c)
different electrons
d)
different protons
36.
How many neutrons does a Sodium 24 isotope have?
a)
12
b)
13
c)
14
d)
15
37.
How many neutrons does a Carbon 13 atom have?
a)
6
b)
5
c)
7
d)
8
38.
How many neutrons does a Calcium 48 isotope have?
a)
16
b)
20
c)
28
d)
12
39.
How many neutrons does an Oxygen-19 isotope have?
a)
19
b)
8
c)
11
d)
10
40.
How many neutrons does an Iodine-133 isotope have?
a)
80
b)
133
c)
53
d)
77
41.
What is the atomic mass of the pictured isotope?
a)
2
b)
4
c)
6
d)
Hehehehe
42.
What is the name of the pictured isotope?
a)
Copper-29
b)
Copper-63
c)
Copper-34
d)
CopperWopperHopperBopper
43.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
44.
Which statement is true according to current thinking?
a)
An atom is mostly empty space.
b)
An atom is a collection of particles, so tightly packed that there is little empty space.
c)
The atomic nucleus is very mobile, and moves around inside a cloud of electrons.
d)
The size of atoms changes over time, pulsating from large to small to large again.
45.
What particle was used in the gold foil experiment?
a)
Beta Particle
b)
Alpha particle
c)
Gamma ray 
46.
Most of the alpha particles went straight through the gold foil.  This suggested that....
a)
There is no interference between alpha and gold.
b)
Most of the atom is made up of empty space.
c)
The alpha particles were very tiny.
d)
None of the above
47.
Some of the alpha particles fired at the gold foil were deflected at angles.  This was due to...
a)
reflection of the alpha source when it it the fluorescent screen.
b)
The alpha particles hitting the gold nucleus.
c)
Repulsion forces between the positively charged nucleus and the positively charged alpha particles. 
d)
A mis-firing of the alpha source
48.

In the 'plum-pudding' model the electrons and found

a)

at the bottom of the ball of positive charge

b)

spread out through out the ball of negative charge

c)

spread out through out the ball of positive charge

d)

all together in the middle

49.

Which scientist discovered the atom has a small central positive nucleus with negative electrons orbiting it?

a)

Bohr

b)

Chadwick

c)

Dalton

d)

JJ Thomson

e)

Rutherford

50.

Bohr discovered that the _________________ are at fixed distances from the nucleus.

a)

protons

b)

neutrons

c)

energy shells

51.
  1. Who first grouped elements in families (similar chemical and physical properties)?
a)

Newlands

b)

Mendeleev

c)

Dobereiner

d)

Moseley

52.

Who arranged the known elements into horizontal rows of increasing atomic mass leaving gaps for as yet undiscovered elements?

a)

Mendeleev

b)

Meyer

c)

Newlands

d)

Moseley

53.
What was Dmitri Mendeleev's greatest contribution to the history of the periodic table?
a)
He arranged all of the known elements by their atomic number
b)
He realised that there was a pattern of reactivity which repeated every 8 elements
c)
He predicted the existence (and properties) of new elements
d)
He identified the "law of triads" which became the groups
54.
The periodic table is organized by the number of ______ in each element's nucleus
a)
neutrons
b)
protons
c)
electrons
d)
atoms
55.
Why were there blank spaces left in Mendeleev's periodic table?                                              
a)
He didn't know what to put there.
b)
 Undiscovered elements not yet known.
c)
Multiple elements could have fit
d)
He forgot to add the elements in.
56.
Mendeleev classified elements based on not only atomic mass but what else?                                                   
a)
reactivity
b)
boiling points
c)
physical properties only 
d)
 chemical & physical properties
57.

Which scientist arranged the 60 known elements in columns of increasing atomic mass so that each column contained seven elements?

a)

Newlands

b)

Meyer

c)

Mendeleev

d)

Moseley

58.

How did Mendeleev overcome some of the problems in his version of the periodic table?

a)

He made up new elements to fill in gaps.

b)

He left gaps for undiscovered elements.

c)

He ordered the elements in terms of atomic mass.

d)

He placed elements in groups according to similar properties.

59.

Magnesium is in Group 3 and Period 2. What is the electronic structure of magnesium?

a)

1.1.1

b)

3.2

c)

2.8.2

d)

2.8.8

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