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Worksheets22 Adv Unit 4 Review
Total questions: 50
Worksheet time: 1hrs 1mins
Name
Class
Date
1.
The early periodic table organized the elements in periods of increasing atomic mass. What information is currently used to organize the elements on the periodic table?
a)
number of valence electrons
b)
number of energy levels
c)
atomic number
d)
ionic radius
2.
The number of valence electrons in an element affects the reactivity of that element. Which element listed has the fewest valence electrons?
a)
beryllium (Be)
b)
sodium (Na)
c)
oxygen (O)
d)
neon (Ne)
3.
According to the Periodic Table of the Elements, which set of elements has similar properties?
a)
H, C, I
b)
He, H, Al
c)
He, Ne, Ar
d)
Na, Ca, Al
4.
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.
5.
Which is larger:
P or P-3
a)
P
b)
P-3
c)
both are same size
6.
Which is larger:
Ca or Ca+2
a)
Ca
b)
Ca+2
c)
both are same size
7.
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
8.
The atom with the largest atomic radius in Group 18 is
a)
Ar
b)
He
c)
Kr
d)
Rn
9.
The element with the largest electronegativity in the halogens is
a)
Cs
b)
F
c)
Fr
d)
O
10.
The element with the lowest electronegativity is
a)
Cs
b)
F
c)
Fr
d)
O
11.
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
12.
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
13.
The elements touching the zig-zag line are called
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
14.
The halogens are ____________.
a)
solids
b)
metalloids
c)
nonmetals
d)
metals
15.
The alkali metals are ______________.
a)
diatomic molecules
b)
metalloids
c)
nonmetals
d)
metals
16.
Noble gases would fit into which group?
a)
metals
b)
nonmetals
c)
metalloids
d)
diatomic molecules
17.
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 neutrons
18.
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.
19.
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)
20.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
21.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
22.
Each column of the Periodic Table is called a...
a)
group
b)
period
c)
metal
d)
mass
23.
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
24.
Which of these elements has the SMALLEST atomic radius?
a)
H hydrogen
b)
Rb rubidium
c)
Li lithium
d)
Fr francium
25.
Which of these elements is the most electronegative?
a)
oxygen O
b)
tellurium Te
c)
Neon Ne
d)
strontium Sr
26.
How many electrons do atoms need to be stable?
a)
1
b)
2
c)
6
d)
8
27.
______ have properties of both metals and non metals, some are semi-conductors, seperates metals from non-metals
a)
Metals
b)
Non-Metals
c)
Metalloids
d)
Groups
28.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals
c)
Alkali Metals
d)
Halogens
29.
Gold, which is in Group 11 on the periodic table, is an example of a(n) ____________
a)
Alkali Metal
b)
Other Metal
c)
Transition Metal
d)
Alkaline Earth Metal
30.
How many elements are in one period in which only the s and p sublevels are completely filled?
a)
2
b)
8
c)
18
d)
32
31.
How do you determine the number of valence electrons an element has?
a)
Look at its period
b)
Look at its group
c)
Look at its atomic number
d)
Look at its atomic mass
32.
How is the modern periodic table set up?
a)
increasing atomic mass only
b)
increasing atomic number only
c)
increasing atomic mass with periods and groups
d)
increasing atomic number with periods and groups
33.
As you move left to right across a period, the atomic radius will ....
a)
decrease
b)
increase
c)
stay the same
34.
Group 17 elements, the halogens, are the most reactive of the nonmetal elements because they
a)
require only one electron to fill their outer
energy level.
energy level.
b)
have the highest ionization energies.
c)
have the largest atomic radii.
d)
are the farthest to the right in the periodic table.
35.
The ________________ determines the position of each element in the periodic table.
a)
mass number
b)
protons
c)
neutrons
d)
valence electrons
36.
The noble gases have
a)
large atomic radii.
b)
very negative electron affinities.
c)
high ionization energies.
d)
a tendency to form both cations and anions.
37.
When an electron is added to a neutral atom, energy is
a)
always absorbed
b)
always released
c)
either absorbed or released
d)
neither absorbed nor released
38.
From left to right across a period on the periodic table, electron affinity values tend to become more
a)
negative
b)
positive
39.
The group of elements that combine with Group 17 elements to form salts is _____.
a)
Alkali Metals
b)
Alkaline Earth Metals
c)
Transition Metals
d)
Metalloids
40.
The groups of elements that are inert because they have full outer energy levels, most of which are gases, are _____.
a)
Alkali Metals
b)
Alkaline Earth Metals
c)
Halogens
d)
Noble Gases
41.
Atoms that lose electrons form positive ions called _____.
a)
anions
b)
cations
c)
protons
d)
neutrons
42.
Which of the following elements would have physical and chemical characteristics similar to sodium?
a)
hydrogen
b)
potassium
c)
magnesium
d)
neon
43.
Which element needs to lose one electron to have an ionic charge of +1?
a)
Lithium
b)
Magnesium
c)
Carbon
d)
Chlorine
44.
Half the distance from the center of one atom to the center of an adjacent like atom is called
a)
Electronegativity
b)
Ionization Energy
c)
Repulsion
d)
Atomic Radius
45.
When oxygen forms an ion, it gains two electrons and has a charge of _____.
a)
+2
b)
-2
c)
+6
d)
-6
46.
Place these elements, Cesium - Strontium - Cadmium - Fluorine in order of electronegativity, from lowest to highest
a)
Cesium - Fluorine - Strontium - Cadmium
b)
Cesium - Strontium - Cadmium - Fluorine
c)
Cadmium - Cesium - Fluorine - Strontium
d)
Fluorine - Cadmium - Strontium - Cesium
47.
Rank these elements in order of their atomic radius, from largest to smallest: Zirconium - Cesium - Nickel - Nitrogen
a)
They are all the same size
b)
Nitrogen - Nickel - Zirconium - Cesium
c)
Nickel - Cesium - Nitrogen - Zirconium
d)
Cesium - Zirconium - Nickel - Nitrogen
48.
The scientist that first developed the basic pattern of the periodic table was _____.
a)
Lavoisier
b)
Davy
c)
Mendeleev
d)
Moseley
49.
Elements that are dull and brittle as solids, and many of which are gases, are the _____.
a)
metals
b)
metalloids
c)
nonmetals
d)
transition metals
50.
Which group of elements is described as shiny, malleable, ductile, and good conductors?
a)
Metals
b)
Halogens
c)
Nonmetals
d)
Noble Gases
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