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Periodic Table and Trends

Total questions: 61

Worksheet time: 53mins

Name
Class
Date
1.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
2.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
3.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
4.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
5.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
6.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
7.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
8.

Ions are formed when atoms gain or lose ___.

a)

electrons

b)

protons

c)

neutrons

d)

atomic mass

9.

What property is being measured in this diagram?

a)

Density

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

10.

If a potassium atom lost one electron, what would be the symbol for that ion?

a)
b)
c)
d)
11.

Which element in period 4 has the highest electronegativity?

a)

potassium

b)

calcium

c)

copper

d)

bromine

12.

The common charge on an atom in group 17 would be....

a)

+1

b)

+7

c)

-7

d)

-1

e)

17

13.

What type of elements are poor conductors of heat and electricity?

a)

transition metals

b)

inner transition metals

c)

metals

d)

nonmetals

14.

What type of elements are malleable and ductile?

a)

noble gases

b)

nonmetals

c)

metals

d)

halogens

15.
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)
16.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

17.

Find an element with similar chemical properties to Barium (Ba)

a)

Ca and Ra, because they are in the same group and have similar chemical properties

b)

Ca and Y, because they are at a 90 degree angle and have similar chemical properties

c)

Cs and La, because they are within the same period

18.

Which of the following could be properties of NONmetals?

a)

Poor electrical conductivity

b)

Dullness

c)

poor thermal conductivity

d)

Brittleness

e)

All the above

19.

True or False: The reactivity of metals tends to decrease as you move RIGHT on the periodic table

a)

False

b)

True

20.

How do you determine the valence electron count of an element?

a)

Protons + Neutrons

b)

Mass# - Electrons

c)

Group #

d)

Proton #

21.

Select the element with the highest ionization energy

a)

Sodium

b)

Aluminum

c)

Phosphorous

d)

Chlorine

22.

Select the element that is a metalloid

a)

Gallium

b)

Boron

c)

Oxygen

d)

Magnesium

23.

Select the element with the highest electronegativity

a)

Chlorine

b)

Silicon

c)

Argon

d)

Magnesium

24.

What element is found in Group 5 period 4?

a)

Zirconium

b)

Magnesium

c)

Strontium

d)

Vanadium

25.

Select the element with the lowest ionization energy.

a)

Barium

b)

Beryllium

c)

Magnesium

d)

Strontium

26.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
27.
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
28.
Define electron affinity.
a)
The energy it takes to add an electron to an atom.
b)
The energy it takes to remove an electron from an atom.
29.
Chlorine and Fluorine are both very electronegative, as they are both missing a single electron from their valence energy level.  Why is Fluorine more electronegative than Chlorine? 
a)
Fluorine has less energy levels.
b)
Chlorine has more electrons in its outer shell
c)
Fluorine has more protons.
d)
None of these
30.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
31.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

32.

Identify the Electron Configuration for Aluminum (Al)

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3p3

c)

1s2 2s2 2p6 3s2 4p1

33.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
34.

Energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

35.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

36.

What is the position of an element in the periodic table if its electron configuration is 1s2 2s2 2p6 3s2 3p5?

a)

Group 1A

b)

Group 2A

c)

Group 5A

d)

Group 7A

37.

Why do electrons enter the 4s orbital before entering the 3d orbital? 

a)

because the 3d orbital is at a lower energy level

b)

because both the 4s and 3d orbitals are at the same energy level

c)

because the 4s orbital is at a lower energy level

d)

because the 4s orbital is at a higher energy level

38.

A particular atom has 8 protons, 8 electrons and 9 neutrons. State its atomic number.

(a)  

39.

What is the overall charge of an atom?

a)

postive

b)

negative

c)

neutral

d)

not sure

40.

How many electrons can the d sublevel hold?

a)
8
b)
10
c)
2
d)
4
41.

What is the maximum number of electrons that an s orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

42.

How many electrons can the p sublevel hold?

a)
8
b)

6

c)
2
d)
4
43.

What is the maximum number of electrons that an f orbital can have?

a)

11 electrons

b)

14 electrons

c)

13 electrons

d)

12 electrons

44.

How many electrons can the third energy level hold?

a)

2

b)

18

c)
8
d)
0
45.

What atom matches this electron configuration?

1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

46.

What element has the electron configuration 

1s22s22p31s^22s^22p^3  

a)

Nitrogen

b)

Oxygen

c)

Magnessium

d)

Carbon

47.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
48.

Which orbital is displayed correctly?

a)

A

b)

B

c)

C

d)

D

49.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
50.

If a neutral Chlorine has an atomic number of 17 and an atomic mass of 35amu, how many protons, neutrons and electrons must it have?

a)

Protons - 17

Neutrons - 17

Electrons - 17

b)

Protons - 35

Neutrons - 35

Electrons - 17

c)

Protons - 17

Neutrons - 18

Electrons - 35

d)

Protons - 17

Neutrons - 18

Electrons - 17

e)

Protons - 18

Neutrons - 35

Electrons - 17

51.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
52.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
53.
[Ne]3s1 is the noble gas configuration for which element?
a)
sodium
b)
lithium
c)
fluorine
d)
aluminum
54.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
55.

What was the identity of the unknown substance?

a)

LiCl

b)

CaCl2

c)

NaCl

d)

BaCl2

e)

SrCl2

56.

A fellow student of yours thought that flame color was based on the element written at the beginning of the compound. Which statement would give evidence to support their claim?

a)

The flames of LiCl and and NaCl are the same color

b)

The flames of LiCl and NaCl are different colors

c)

The flames of Na2SO4 and NaCl are different colors

d)

The flames of Na2SO4 and CuCl2 are different colors

57.

Which scientific principle would be most useful to connect your claim to your evidence in this lab?

a)

Chemical properties can only be observed by changing the identity of the substance

b)

A chemical change results in a new substance

c)

A physical change does not produce a new substance

d)

Physical properties can be observed without changing the identity of the substance

58.

Why do we wet the cotton swap before dipping it into the salt?

a)

to clean the cotton swab

b)

to make the salt stick to it

c)

to prevent the cotton swab from burning

d)

all of these are true

59.

An atomic emission spectrum is...

a)

unique to the element

b)

a complete rainbow

c)

both of these are correct

d)

neither of these are correct

60.

Light of a specific frequency is emitted when...

a)

an electron absorbs energy

b)

an electron moves down an energy level

c)

when an electron gets excited

d)

all of these are true

61.

A practical application of atomic emission spectra is ....

a)

neon lights

b)

fireworks

c)

identifying unknown substances

d)

all of these

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