NEW
Font size
S
M
L
XL
WorksheetsAccel-Unit 2- Periodic Table & Electrons
Total questions: 30
Worksheet time: 31mins
Name
Class
Date
1.
What do the periods on the periodic table tell you?
a)
electrons
b)
sublevels
c)
energy levels
2.
What do the elements in the same group have in common?
a)
properties & valence electrons
b)
energy level & valence electrons
c)
protons & valence electrons
3.
Ionization Energy is
a)
the energy required to remove an electron
b)
the ability to attract electrons
c)
half the distance between the nuclei of 2 adjacent atoms
d)
half the distance between the nuclei of 2 ions
4.
What happens to the radius of an atom when it becomes a cation?
a)
gets bigger because less electrons, so less electron repulsion
b)
gets smaller because less electrons, so less electron repulsion
c)
gets bigger because more electrons, so more electron repulsion
d)
gets smaller because more electrons, so more electron repulsion
5.
What happens to the radius of an atom when it becomes an anion?
a)
gets bigger because less electrons, so less electron repulsion
b)
gets smaller because less electrons, so less electron repulsion
c)
gets bigger because more electrons, so more electron repulsion
d)
gets smaller because more electrons, so more electron repulsion
6.
Atomic radius ______ left to right across a period and ______ down a group
a)
decreases, increases
b)
increases, decreases
7.
Electronegativity is
a)
the energy required to remove an electron
b)
the ability to attract electrons
c)
half the distance between the nuclei of 2 adjacent atoms
d)
half the distance between the nuclei of 2 ions
8.
Atomic radius _________ across a period because __________.
a)
decreases; energy levels and electron shielding increases
b)
decreases; nuclear charge (more protons) increases
c)
increases; energy levels and electron shielding increases
d)
increases; nuclear charge (more protons) increases
9.
Put the elements below in order of increasing ionization energy: K, Ti, Cs
a)
Cs, Ti, K
b)
Ti, K, Cs
c)
Cs, K, Ti
d)
Ti, K, Cs
10.
What happens to the atomic radius as you go down a group?
a)
gets smaller because the effective nuclear charge gets bigger
b)
gets bigger because the effective nuclear charge gets smaller
c)
gets smaller because of an increase in electron shielding
d)
gets bigger because of an increase in electron shielding
11.
Which group of metals on the periodic table is more reactive?
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
inner transition metals
12.
Which group of elements has no electronegativity values?
a)
alkali metals
b)
halogens
c)
noble gases
d)
alkaline earth metals
13.
Elements gain or lose electrons to form…..
a)
atoms
b)
ions
c)
isotopes
d)
neutral
14.
What do halogens do when they form ions? What kind of charge does this give them?
a)
gain an electron; - charge
b)
lose an electron; + charge
c)
gain 2 electrons; 2+ charge
d)
lose 2 electrons; 2- charge
15.
What would be the charge on an ion of Ca?
a)
Ca-
b)
Ca2-
c)
Ca+
d)
Ca2+
16.
What kind of charge do the alkali metals have when they form ions?
a)
+
b)
2+
c)
-
d)
2-
17.
Write the electron configuration for Br. What energy level are the valence electrons in?
a)
1s22s22p63s23d103p6;3 energy level
b)
1s22s22p63s23p64s23d104p6; 4th energy level
c)
1s22s22p63s23p64s23d104p5; 4th energy level
d)
1s22s22p63s23d103p5;3 energy level
18.
What is this element?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
19.
What is this element?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
20.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
21.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
22.
What is this element?
[Ne] 3s23p64s2
[Ne] 3s23p64s2
a)
Calcium
b)
Sodium
c)
Scandium
d)
Titanium
23.
Which sub-level can hold up to 6 electrons?
a)
s
b)
p
c)
d
d)
f
24.
How many electrons can a single p orbital hold?
a)
1
b)
2
c)
3
d)
6
25.
Given the spectrum, which elements are present in the mixture?
a)
Li & Cd
b)
Sr & Li
c)
Cd & Sr
26.
Write the electron configuration for P3-.
a)
1s22s22p63s23p3
b)
1s22s22p6
c)
1s22s22p3
d)
1s22s22p63s23p6
27.
The letter "n" represents
a)
sublevels
b)
energy levels
c)
electrons
d)
orbitals
28.
What is the shape of a p sublevel?
a)
sphere
b)
dumbbell
c)
varied
29.
Electrons with opposite spins are located in
a)
orbitals
b)
orbits
c)
planets
30.
What is the noble gas configuration for Ti+2?
a)
1s22s22p63s23p64s23d2
b)
[Ar]4s23d2
c)
[Ar]3d2
d)
[Ar]4s2
Reset
