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WorksheetsPeriodic Table & Trends
Total questions: 54
Worksheet time: 4hrs 0mins
Name
Class
Date
1.
A horizontal row of elements in the periodic table.
a)
column
b)
group
c)
period
2.
A vertical column in the periodic table. Elements share similar properties.
a)
row
b)
group
c)
period
3.
How did Mosely set up the modern periodic table?
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
4.
Elements in a ..................have similar chemical properties.
a)
period
b)
group
c)
row
5.
States repeating properties of element change with atomic numbers.
a)
group
b)
period
c)
periodic law
6.
As you move from left to right across a period, the atomic number will ....
a)
decrease by 1 from element to element
b)
decrease by 2 from element to element
c)
increase by 1 from element to element
d)
increase by 2 from element to element
7.
As you move left to right across a period, the atomic radius will ....
a)
decrease
b)
increase
c)
stay the same
8.
As you move from Carbon to Nitrogen, the atomic radius will ....
a)
decrease
b)
increase
c)
stay the same
9.
As you move from Beryllium to Lithium, the atomic radius will ...
a)
decrease
b)
increase
c)
stay the same
10.
As you move down a group, the atomic radius will ....
a)
decrease
b)
increase
c)
stay the same
11.
How did Mendeleev organize the elements in his periodic table?
a)
increasing mass only
b)
increasing atomic number only
c)
increasing atomic mass with periods and groups
d)
increasing atomic mass with periods and groups
12.
_______________ developed the first periodic table and arranged the elements in order of increasing atomic mass.
a)
Stevie Wonder
b)
Sasha Vujacic
c)
Dmitri Mendeleev
d)
James Mosely
13.
Name the most abundant (the most ) elements on the periodic table.
a)
gold
b)
metals
c)
nonmetals
d)
metalloids
14.
Which are good conductors of electricity? (metals, metalloids, or non-metals)
a)
metals
b)
metalloids
c)
nonmetals
15.
Which of these is a property of metals that can be used to identify them as metals rather than nonmetals.
a)
dull
b)
slimy
c)
malleable
d)
bad conductor of electricity
16.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
17.
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)
18.
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
19.
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.
20.
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.
21.
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
22.
The atom with the largest atomic radius in Group 18 is -
a)
Ar
b)
He
c)
Kr
d)
Rn
23.
The tendency of an atom to attract electrons and acquire a negative charge
a)
electronegativity
b)
charge
c)
bonding ability
d)
electron configuration
24.
All alkali metals have --------------- electrons in their outermost shell.
a)
1
b)
2
c)
3
d)
4
25.
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
26.
In what section would Noble Gases be found?
a)
white
b)
yellow
c)
blue
d)
red
27.
Which element is not a metal?
a)
H
b)
Re
c)
Al
d)
B
28.
Why are elements in groups 1 and 17 highly reactive?
a)
Because they don't bond with other elements
b)
Because they have 8 valence electrons and are stable
c)
Because they loose/gain 1 valence electron
d)
None of the above
29.
How many electrons do atoms need to be stable?
a)
1
b)
2
c)
6
d)
8
30.
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)
31.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium
c)
francium
d)
cesium
32.
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
33.
Which of the following is arranged according increasing reactivity?
a)
Mg > Li > Na > K
b)
Mg > Na > Li > K
c)
Na > Li > Mg > K
d)
K > Mg > Na > Li
34.
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)
Other Metals
35.
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
36.
If a material can easily be drawn into the shape of a wire, it is
a)
reactive
b)
magnetic
c)
malleable
d)
ductile
37.
As you move down the first group, reactivity _________.
a)
Increases
b)
Decreases
c)
Stays the same
d)
They are all inert
38.
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
39.
Which is a chemical property of metals
a)
malleable
b)
ductile
c)
reactivity
d)
luster
40.
Insulators, brittle, dull, crumbly, tends to gain electrons, mostly gasses at room temperature, located on the right.
a)
Metals
b)
Non-Metals
c)
Metalloids
d)
Periods
41.
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
42.
What happens when cesium forms an ion?
a)
gains one electrons
b)
loses two electrons
c)
gains three electrons
d)
loses one electron
43.
What happens when magnesium forms an ion?
a)
gains two electrons
b)
loses two electrons
c)
gains three electrons
d)
loses one electron
44.
Cations are
a)
positive
b)
negative
c)
on the right side of the periodi table.
d)
nonmetals
45.
Which of the following would produce an anion?
a)
Ca
b)
Al
c)
K
d)
F
46.
What will nitrogen's charge be as an ion?
a)
+3
b)
-3
c)
0
d)
-1
47.
Cations are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
48.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
49.
Ions are:
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
50.
Sodium is in group 1 of the Periodic Table. What is the formula of the ion?
a)
Na2-
b)
Na2+
c)
Na+
d)
Na-
51.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
52.
Magnesium's ion
a)
Mg+
b)
Mg2+
c)
Mg-
d)
Mg2-
53.
What charge will an Oxygen ion have?
a)
+1
b)
-1
c)
+2
d)
-2
54.
What is the charge does a sodium ion have?
a)
+2
b)
+1
c)
-1
d)
-2
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