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OC Summer Chem Unit 6

Total questions: 23

Worksheet time: 3615secs

Name
Class
Date
1.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

2.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

3.

Vertical columns on the periodic table are called ___?

a)

groups

b)

periods

c)

rows

d)

families

4.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
5.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
6.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
7.
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
8.
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
9.

What is a positively-charged ion which forms when an atom loses electrons?

a)

atom

b)

ion

c)

cation

d)

anion

10.
What is the family name of this group of elements? 
a)
Alkali metals 
b)
Halogens 
c)
Noble Gases 
d)
Alkali Earth Metals 
11.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
12.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
13.
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. 
14.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
15.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
16.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
17.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
18.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

19.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

20.

Which of the following is not a correct designation for a sublevel?

a)

zz

b)

p

c)

d

d)

f

21.

Match the elements with their electron configuration! (3 minutes)

a)

1s2 2s2 2p3

1.

Nitrogen, N

b)

1s2 2s2 2p6 3s2 3p3

2.

Phosphorus, P

c)

1s2

3.

Helium, He

d)

1s2 2s2 2p6 3s2 3p6

4.

Argon, Ar

e)

1s2 2s2 2p6 3s2

5.

Magnesium, Mg

22.
What does Hund's rule states ?
a)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
23.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

There is nothing incorrect with this diagram

c)

In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box pointing in the same direction.

d)

All the arrows should be pointing up.

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