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Periodic Trends 1

Total questions: 50

Worksheet time: 49mins

Name
Class
Date
1.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
2.

The atom with the largest atomic radius in Group 18 is -

a)

Ar

b)

He

c)

Kr

d)

Rn

3.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
4.

The atom with the largest atomic radius in Period 4 (row 4) is -

a)

K

b)

Kr

c)

Fe

d)

Fe

5.
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, so little energy is needed to remove it
6.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
7.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
8.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
10.
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
11.

Which of the following will have a larger radius than Zinc?

a)

Gallium

b)

Aluminum

c)

Magnesium

d)

Strontium

12.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

13.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
14.

Which general trend exists for ionization energy when moving left to right across a period?

a)

Ionization energy first increases then decreases

b)

Ionization remains fairly constant.

c)

Ionization energy increases

d)

Ionization energy decreases

15.

Which group tends to have the highest ionization energy? The lowest?

a)

Group 7; Group 2

b)

Group 1; Noble gases

c)

Group 2; Group 7

d)

Group 7; Group 1

16.

Electronegativity of an element generally __________ as you move down a group in the periodic table.

a)

remains unchanged

b)

fluctuates

c)

increases

d)

decreases

17.

Why do noble gases lack electronegativity values?

a)

they don’t readily bond with other atoms

b)

they have a completely filled valence electron shell

c)

they have a partially filled valence electron shell

d)

they don’t have a valence electron electrons

18.

Which of the following elements has the LARGEST atomic radius?

a)

K

b)

Na

c)

Al

d)

N

19.

Which of the following elements is the LEAST electronegative?

a)

Be

b)

Rb

c)

O

d)

B

20.
The ionization potential of an element is the amount of energy required to remove an electron from an isolated atom or molecule. According to the periodic table, which of the following indicates the correct decreasing order of ionization energy?
a)
Li > Na > K > Cs
b)
Na > K > Li > Cs
c)
Li > K > Na > Cs 
d)
Cs > K > Na > Li 
21.

Which of the following elements has the smallest atom?

a)

Na

b)

Mg

c)

Cl

d)

Si

22.

Which of the following elements has/have lower electron affinity than fluorine atom?

a)

Aluminum

b)

Magnesium

c)

Selenium

d)

Options 1, 2 and 3

23.

Which of the following periodic properties increases across a period from left to right?

I. Atomic radii

II. Electronegativity

III. First ionization energy

a)

I only

b)

II only

c)

I and II only

d)

II and III only

24.

The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.

Which element has the highest electronegativity?

a)

W

b)

X

c)

Y

d)

Z

25.

Order the elements S, Cl, and F in terms of increasing atomic radii.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

26.

Choose the element with the highest ionization energy.

a)

Na

b)

Mg

c)

Al

d)

P

e)

S

27.

Which of these has the most electron affinity?

a)

Sulfur S

b)

Tin Sn

c)

Barium Ba

d)

Iodine I

28.

Which of these has the most electron affinity?

a)

Cesium Cs

b)

Yittrium Y

c)

Nitrogen N

d)

Neon Ne

29.

Which one of these has the lowest electron affinity?

a)

Bismuth Bi

b)

Gold Au

c)

Osmium OS

d)

Barium Ba

30.

Electron affinity is the ability for an atom to ____________ another electron.

a)

Keep

b)

Attract

c)

Repulse

31.

The reason why Fluorine will steal another electron is because ___________.

a)

It will increase the potential energy in Fluorine

b)

It will decrease the potential energy in Fluorine

c)

It will make Fluorine more stable

d)

Both decrease PE and make it stable

e)

Both Increase PE and make it stable

32.

Metals tend to make positive ions because _________________.

a)

They have lower electronegative values

b)

They have high electronegative values

c)

They have smaller radii than non metals

d)

They have high ionization energies

33.

Positive ions are usually ____________ than atoms of the same element.

a)

Stronger

b)

Weaker

c)

Smaller

d)

Bigger

34.

Negative ions (anions) are usually ______________ than atoms of the same element.

a)

Stronger

b)

Weaker

c)

Smaller

d)

Bigger

35.

Electronegativity is a combination of ___________________ and ____________________.

a)

I Atomic Radius

b)

II Ionization Energy

c)

III Electron Affinity

d)

Both II & III

36.

Which of these has the largest atomic radius?

a)

Sodium Na

b)

Aluminum Al

c)

Phosphorus P

d)

Argon Ar

37.

Which of these has the largest atomic radius?

a)

Beryllium Be

b)

Radium Ra

c)

Strontium Sr

d)

Calcium Ca

38.

Which of these has the largest ionization energy?

a)

Potassium K

b)

Iron Fe

c)

Zinc Zn

d)

Selenium Se

39.

Which of these has the lowest ionization energy?

a)

Fluorine F

b)

Chloride Cl

c)

Bromine Br

d)

Iodine I

40.

Which one of these has the highest electron affinity?

a)

Magnesium Mg

b)

Aluminum Al

c)

Phosphorus P

d)

Chlorine Cl

41.

Which of these has the lowest electron affinity?

a)

Gallium Ga

b)

Indium In

c)

Boron B

d)

Aluminum Al

42.

Which of these has the highest Electronegativity?

a)

Cesium Cs

b)

Cobalt Co

c)

Oxygen O

d)

Silicon Si

43.

Which of these has the lowest Electronegativity?

a)

Arsinic As

b)

Barium Ba

c)

Carbon C

d)

Mercury Hg

44.

If the difference in Electronegativity is between 0.5 and 2, the the type of bond between atoms will be _________________.

a)

Non polar Covalent

b)

Polar Covalent

c)

Ionic

d)

Metallic

45.

If the difference in Electronegativity between two atoms is above 2 then the bond between atoms is _________________.

a)

Non polar covalent

b)

Polar covalent

c)

Ionic

d)

Metallic

46.

If the difference in Electronegativity between two atoms is less than 0.5 then the bond between the atoms will be _______________.

a)

Non polar Covalent

b)

Polar covalent

c)

Ionic

d)

Metallic

47.

Which of these has the smallest atomic radius?

a)

Oxygen O

b)

Helium He

c)

Tin Sn

d)

Magnesium Mg

48.

Which of these has the lowest ionization energy?

a)

Iodine I

b)

Zinc Zn

c)

Rubidium Rb

d)

Sodium Na

49.

Which of these has the highest Electronegativity?

a)

Sulfur S

b)

Chlorine Cl

c)

Bromine Br

d)

Tellurium Te

50.

If Sodium has an electronegativity of 0.9 and Chloride has an electronegativity of 3.5, what type of bond is between Sodium and Chloride?

a)

Non polar covalent

b)

Polar covalent

c)

Ionic

d)

Metallic

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