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Review- Atoms, Periodic Table

Total questions: 76

Worksheet time: 1hrs 4mins

Name
Class
Date
1.

Put these elements in order of INCREASING atomic radius.

Li, O, C, F

a)

O, C, F, Li

b)

F, O, C, Li

c)

Li, C, O, F

d)

C, F, Li, O

2.

Put these elements in order of DECREASING atomic radius.

Ca, Be, Ba, Sr

a)

Sr, Ba, Be, Ca

b)

Be, Ca, Sr, Ba

c)

Ba, Sr, Ca, Be

d)

Ca, Be, Ba, Sr

3.

As you move left to right on a period, the force which attracts electrons gets (a)   .

4.

Why do metals become more reactive as they move down a group?

a)

they have the same number of electrons

b)

they have the same number of orbits

c)

the electrons are further from the pull of the proton

d)

the electrons are closer to the nucleus

5.

What is the trend for atomic radius down a group?

a)

The atomic radius increases

b)

the atomic radius decreases

c)

the atomic radius stays the same

d)

the atomic radius is not a trend

6.

Reorder the following by increasing size.

a)

lithium

b)

sodium

c)

potassium

d)

rubidium

e)

cesium

1)
2)
3)
4)
5)
7.

What is electronegativity?

a)

The ability of an atom to attract and bind with electrons

b)

The energy needed for a neutral atom to remove an electron

c)

The ability of an atom to become a negative ion

d)

The size of an atom

8.

Which element has the least electronegativity?

a)

Francium

b)

Cesium

c)

Fluorine

d)

Helium

9.

What is ionization energy?

a)

The ability of an atom to attract and bind with electrons

b)

The energy needed for a neutral atom to remove an electron

c)

The ability of an atom to become a negative ion

d)

The size of an atom

10.

Which element has the highest ionization energy?

a)

Francium

b)

Cesium

c)

Fluorine

d)

Helium

11.

What is electron affinity?

a)

The ability of an atom to attract and bind with electrons

b)

The energy needed for a neutral atom to remove an electron

c)

The ability of an atom to become a negative ion

d)

The size of an atom

12.

What is atomic radius?

a)

The ability of an atom to attract and bind with electrons

b)

The energy needed for a neutral atom to remove an electron

c)

The ability of an atom to become a negative ion

d)

The size of an atom

13.

What is the trend of atomic radius across a period in the periodic table?

a)

Increases

b)

Decreases

c)

Remains constant

d)

First increases, then decreases

14.

What is the trend of electronegativity down a group in the periodic table?

a)

Increases

b)

Decreases

c)

Remains constant

d)

First increases, then decreases

15.

What is the trend of ionization energy down a group in the periodic table?

a)

Increases

b)

Decreases

c)

Remains constant

d)

First increases, then decreases

16.

Which element has the lowest electron affinity?

a)

Francium

b)

Cesium

c)

Fluorine

d)

Helium

17.

Why does radius decrease as you move across a period?

a)

because electrons are being added

b)

because protons are being added

c)

because energy levels are being lost

d)

because energy levels are being added

18.

The ability of an atom to attract another atom's electrons to itself is called

a)

electronegativity

b)

ionization energy

c)

periodic trend

d)

coulombic attractin

19.

Which group of elements has the lowest ionization energies?

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Halogens (Group 17)

d)

Noble Gases (Group 18)

20.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

21.

What is a vertical (up and down) column in the periodic table?

a)

group or family

b)

period

c)

periodic law

d)

octet rule

22.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
23.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
24.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
25.
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. 
26.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
27.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
28.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
29.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

30.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
31.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
32.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
33.
Atomic Radius is...
a)
the relative size of the atom's nucleus
b)
the relative size of the atom's electron cloud
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
34.
What term is used to describe "A measure of the size of an atom"
a)
chemical reactivity
b)
atomic radius
c)
energy levels
d)
orbit
35.
Looking at atoms in the same group/family, what factor affects Coulombic attraction?
a)
number of protons
b)
distance from the nucleus
36.
Looking at atoms in the same valence energy level, what factor affects Coulombic attraction?
a)
number of protons
b)
distance from the nucleus
37.
As the Coulombic attraction increases the atomic radius: increases or decreases?
a)
increases
b)
decreases
38.
As the Coulombic attraction in an atom increases, the energy needed to remove an electron: increases or decreases?
a)
increases
b)
decreases
39.
As the Coulombic attraction of an atom increases, the electronegativity of the atom: increases or decreases?
a)
increases 
b)
decreases
40.

What idea is this cartoon showing?

a)

chlorine is more electronegative than hydrogen

b)

chlorine has more energy levels than hydrogen

c)

hydrogen is more electronegative than chlorine

41.

Which charge is POSITIVE?

a)

Proton

b)

Neutron

c)

Electron

d)

Cell

42.

All of the ROWS on the Periodic Table are called what?

a)

Periods

b)

Groups

c)

Columns

d)

Lines

43.

What is the ATOMIC # (number on top) of Oxygen- O?

a)

6

b)

7

c)

8

d)

9

44.

How many PROTONS & ELECTRONS does Neon- Ne have?

a)

7

b)

8

c)

9

d)

10

45.

How many PROTONS / ELECTRONS does Potassium- K have?

a)

11

b)

19

c)

37

d)

87

46.

Column / Group 2 on the Periodic Table has what family name?

a)

Alkali Metals

b)

Alkali Earth Metals

c)

Halogens

d)

Noble Gases

47.

The NOBLE GASES are considered:

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

None

48.

Which TWO particles are found housed in the nucleus of the atom?

a)

Protons and Electrons

b)

Protons and Neutrons

c)

Electrons and Neutrons

d)

Protons, Neutrons, and Electrons

49.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

50.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

51.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

52.

12 protons and 13 neutrons

a)

Mg-12

b)

Mg-13

c)

Mg-25

d)

Mg-24.305

53.

Label the two parts of the atom here.

a)Nucleus
b)Electron cloud
1
2
1)
2)
54.

Match the following mass amounts with the proper charge.

a)

Protons

1.

(+)positive

b)

Electron

2.

(-) negative

c)

Neutron

3.

(0) neutral, no charge

55.

The atomic mass of an element is the ____.

a)

total mass of the isotopes of the element

b)

total number of subatomic particles in its nucleus

c)

weighted average of the masses of the isotopes of the element

d)

average of the mass number and the atomic number for the element

56.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
57.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
58.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
59.

Democritus thought matter was made of indestructible particles called

(a)  

60.

What conclusion did Thomson make?

a)

cathode ray tubes are cool

b)

matter must contain negatively charged particles

c)

matter must contain positively charged particles

61.

Which scientist is given credit for discovering the electron?

a)

Bohr

b)

Dalton

c)

Thomson

d)

Rutherford

62.

Who discovered that electrons travel in specific orbits around the nucleus?

a)

Bohr

b)

Schrodinger

c)

Democritus

d)

Rutherford

63.

Whose model of the atom is known as the "plum pudding" model (aka the "chocolate chip cookie" model)?

a)

Rutherford

b)

Schrodinger

c)

Dalton

d)

Thomson

64.

Whose gold foil experiment led to his conclusion that the nucleus of an atom contained protons?

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Dalton

65.

Whose model of the atom is represented in the image?

a)

Thomson

b)

Bohr

c)

Dalton

d)

Rutherford

66.

What is Neils Bohr's contribution to the atomic theory?

a)

Created the atomic theory

b)

Created a model of the atom with electrons moving around the nucleus in a fixed orbits

c)

Discovered that the proton had a positive charge

d)

Believed that atoms of a given element are identical

e)

Discovered the electron

67.

What were Ernest Rutherford's three contributions to atomic theory?

a)

Discovered that the atom is mostly empty space

b)

Discovered the nucleus- did the gold foil experiment

c)

Used the cathode ray tube in his discovery

d)

Discovered the electron

e)

Discovered that the proton had a positive charge

68.
Which scientist saw the atom as a solid sphere?
a)
Dalton
b)
Thomson
c)
Rutherford
d)
Bohr
69.
Proposed electrons move around the nucleus in shells
a)
James Chadwick
b)
J.J. Thomson
c)
Niels Bohr
d)
Ernest Rutherford
70.
Rutherford’s experiment determined that the nucleus of an atom is tiny, dense and  ______ charged. 
a)
neutrally
b)
negatively
c)
positively
71.

Mass is neither created nor destroyed during chemical reactions or physical changes.

a)

Law of multiple proportions

b)

law of definite proportions

c)

law of scientific theory

d)

law of conservation of mass

72.

The atomic number is always equal to the number of:

a)

Neutrons

b)

Electrons

c)

Protons

d)

Positrons

73.

If an electrically neutral element has 10 protons and 12 neutrons, how many electrons does it have?

a)

10

b)

12

c)

22

d)

2

74.

Mass of a proton is the same as the mass of:

a)

electron

b)

neutron

75.

Subatomic particle with the least mass:

a)

Electron

b)

Proton

c)

Neutron

76.

When an electron moves from ground to excited state, the electron

a)

absorbs energy and moves to a higher level (shell)

b)

absorbs energy and moves to a lower level (shell)

c)

releases energy and moves to a higher level (shell)

d)

releases energy and moves to a lower level (shell)

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