Download d. Group 1

Grudge Ball
This is a measure of the energy
required to remove an electron
from an atom.
a. Electron affinity
b. Electronegativity
c. Ionization energy
d. Valence energy
2
c. Ionization Energy
3
What happens to atomic radius
going across the periodic table
from left to right. Why?
a. Radius increases
b. Radius decreases
c. Radius stays the same
4
b. Decreases
5
Which group of elements are likely to
form negative ions (gain electrons)?
a. Groups 1 and 2
b. Groups 3-12
c. Groups 13-15
d. Groups 16 - 17
6
d. Groups 16 and 17
7
Which of the following statements
about ionization energy is correct?
a. Metals have low IE and
nonmetals have high IE
b. Nonmetals have low IE and
metals have high IE
c. Relative IE varies for metals and
nonmetals
8
a.
High IE – Nonmetals
Low IE - Metals
9
Which halogen has the highest
electron affinity?
a. F
b. Cl
c. I
d. At
10
a. Fluorine
11
Where are the most active metals
found on the periodic table?
What do we call them?
a. Group 17: halogens
b. Groups 3-12: transition metals
c. Group 2: alkaline earth metals
d. Group 1: alkali metals
12
d. Group 1: Alkali metals.
13
Which family has a valence level
electron configuration of s2 p5?
Where are they found?
a. Nitrogen family
b. Oxygen family
c. Halogen family
d. Noble gas family
14
c. Halogens.
Group 17
15
Which alkali metal has the largest
atoms?
a. Hydrogen
b. Lithium
c. Francium
d. Radium
16
c. Francium
(Fr)
17
What sublevels are the last to be
filled for the lanthanides and
actinides?
a. s
b. p
c. d
d. f
18
d. f sublevels
(4f and 5f, respectively)
19
Which TWO groups contain the
most reactive elements?
a. Groups 1 and 2
b. Groups 1 and 17
c. Groups 17 and 18
d. Groups 1 and 18
20
b. Groups 1 and 17
Alkali Metals and
Halogens
21
What is the name of the element in
group 17 row 3?
a. Actinium
b. Bromine
c. Chlorine
d. Sulfur
22
c. Chlorine (Cl)
23
The modern periodic law states
that properties of elements are a
periodic function of their ______.
a. Atomic number
b. Atomic mass
c. Atomic structure
d. Atomic periodicity
24
a. atomic number
25
As you move from left to right
through the transition elements in
the fourth row, which energy level
are additional electrons placed in?
a. 3p
b. 3d
c. 4d
d. 4f
26
b. Energy level Three
(3d)
27
In the modern periodic table,
elements are arranged according
to
a. Decreasing atomic mass
b. Mendeleev’s original model
c. Increasing atomic number
d. When they were discovered
c. Increasing atomic number
Why are the noble gases nonreactive?
a. They have no valence electrons
b. They have full electron orbitals
c. They have the most protons
d. They have low ionization energy
30
b. They have full
electron orbitals
They have an octet
(8 valence electrons)
31
Group 17 elements, the halogens,
are the most reactive of the
nonmetal elements because they
a.
b.
c.
d.
Require only one electron to fill their outer
energy level
Have the highest ionization energies
Have the largest atomic radii
Are the farthest to the right in the periodic
table
32
a. Require only one electron to
fill their outer energy level
33
Selenium is in the oxygen family
and period 4. What is the electron
configuration for its outermost
energy level?
a. 4p4
2
4
b. 4s 4p
4
c. 4p
d. [Ar]4s24p4
34
2
b. 4s
4
4p
35
The electron configuration of this
2
2
element ends with 5s 4d .
a. Ti
b. Sr
c. Y
d. Zr
36
d. Zirconium (Zr)
37
How many valence electrons do the
halogens have?
a. 1
b. 2
c. 7
d. 8
38
c. 7
39
a.
b.
c.
d.
Which of these has the
highest energy?
5s
5p
4d
4f
40
d. 4f
41
Which noble gas has the
smallest atom?
a. H
b. He
c. Fr
d. Rn
42
b. Helium
43
Which family of elements typically
has the highest ionization energies?
a. Alkali metals
b. Alkaline earth metals
c. Halogens
d. Noble gases
44
d. Noble gases
45
Identify the largest
a. Na
b. Mg
c. K
46
c) K
47
Which of these is a
metalloid?
a. Al
b. As
c. Ar
d. Ag
48
b. As
(Arsenic)
49
Which is more active?
a. K
b. Na
c. Li
50
a. K
It is larger; the valence
electrons are farther
from the nucleus.
51
In developing his periodic table,
Mendeleev listed on cards each element’s
name, atomic mass, and
a.
b.
c.
d.
atomic number.
electron configuration.
isotopes.
properties.
d. properties.
Mendeleev’s periodic table did not list all
elements in order of increasing atomic
mass because he grouped together
elements with similar
a.
b.
c.
d.
properties.
atomic numbers.
names.
isotopes.
a.
properties
Mendeleev predicted that the
gaps in his periodic table
represented
a.
b.
c.
d.
ions.
radioactive elements.
unstable elements.
undiscovered elements.
d. undiscovered elements.
The person whose work led to a
periodic table based on increasing
atomic number was
a.
b.
c.
d.
Moseley.
Mendeleev.
Rutherford.
Cannizzaro.
a. Moseley
The periodic law states that the
physical and chemical properties of
elements are periodic functions of
their atomic
a.
b.
c.
d.
masses.
numbers.
radii.
structures.
b. numbers.
As you move left to right across period
3 form Mg to Cl, the energy needed to
remove an electron from an atom
(ionization energy)
a.Generally increases
b.Generally decreases
c.Does not change
d.Varies unpredictably
a. Generally increases
A repeating pattern is referred to
as
a.
b.
c.
d.
unpredictable.
irregular.
periodic.
a group.
c. Periodic
On most periodic tables, the lanthanides and
actinides appear
a.
b.
c.
d.
on a separate page.
below the main portion.
on the back.
at the top.
b. Below the main
portion
What is the difference in atomic
number between He and Ne?
a. 2
b. 8
c. 18
d. 32
b. 8
Which noble gas has the
greatest atomic number?
a. Ar
b. Xe
c. Kr
d. Rn
d. Rn
An element that has the electron
configuration [He]2s22p2 is in Period
a.
b.
c.
d.
2.
3.
5.
7.
a. 2
An element that has the electron
configuration [He]2s22p2 is in Group
a.
b.
c.
d.
2.
5.
14.
17.
c. 14.
Elements in the s and p blocks of
the periodic table are called
a.
b.
c.
d.
alloys.
main-group elements.
metals.
transition metals.
b. main-group elements.
Elements in Group 18 have
a.
b.
c.
d.
very low reactivity.
good conductivity.
very high reactivity.
metallic character.
a. very low reactivity.
Nonmetallic elements in Group 17
that react with most metals to
form salts are
a.
b.
c.
d.
alkali metals.
halogens.
lanthanides.
noble gases.
a. alkali metals.
The outer-level electron configuration of
a neutral halogen non-metal atom
consists of
a.
b.
c.
d.
one electron in the s orbital.
five electrons in the s orbital.
one electron in the p orbital.
five electrons in the p orbital.
d. seven electrons in the
p orbital.
In nature the alkali metals are found
only in compounds because they
a.
b.
c.
d.
have small atoms.
are very reactive elements.
are rare elements.
each have a stable octet.
b. are very reactive
elements.
To which group does hydrogen
belong?
a.
b.
c.
d.
Group 1
Group 2
Group 18
None
d. none
An element found in groups 312 of
the periodic table is classified as a(n)
a.
b.
c.
d.
alkali metal.
alloy.
transition metal.
actinide.
c. transition metal.
In which group is an element that has an
outer-level electron configuration
consisting of one electron in the d orbital
and two electrons in the ns orbital?
a.
b.
c.
d.
Group 1
Group 2
Group 3
Group 5
c. Group 3
An electron that is in the highest energy
level of an atom and determines the
atom’s chemical properties is called a(n)
a.
b.
c.
d.
valence electron.
paired electron.
extra electron.
opposite-spin electron.
a. valence electron.
What can be removed from an atom
if ionization energy is supplied?
a.
b.
c.
d.
a proton
a neutron
an electron
an ion
c. an electron
Across a period in the periodic
table, ionization energy generally
a.
b.
c.
d.
decreases.
decreases, then increases.
increases.
remains constant.
c. increases.
Down a group in the periodic table, the
change in ionization energy is due to
a.
b.
c.
d.
increasing electron shielding.
decreasing charge of the nucleus.
increasing neutrons in nucleus.
decreasing atomic radii.
a. increasing electron
shielding.
The atomic radius of an atom that is
chemically bonded to an identical atom is
equal to
a. the distance between the nuclei.
b. half the distance between the
nuclei.
c. twice the distance between the
nuclei.
d.one-fourth the distance between the
nuclei.
b. half the distance
between the nuclei.
Across a period in the periodic
table, atomic radii generally
a.
b.
c.
d.
decrease.
decrease, then increase.
increase.
increase, then decrease.
a. decrease.
Down a group in the periodic
table, atomic radii generally
a.
b.
c.
d.
decrease.
remain constant.
increase.
vary unpredictably.
c. Increases
One of the least electronegative
elements would be found on the
periodic table in
a.
b.
c.
d.
Group 1, Period 7.
Group 3, Period 4.
Group 5, Period 3.
Group 17, Period 2
a. Group 1, Period 7.
As the atomic numbers of the
metals of Group 1 increase, the
ionic radii
a. increase.
b. decrease.
c. remain the same.
d. cannot be determined.
a. increase.
An element with the smallest anionic (negativeionic) radius would be found on the periodic
table in
a.
Group 1, Period 7.
b.
Group 3, Period 4.
c.
Group 5, Period 3.
d.
Group 17, Period 2.
d.
Group 17, Period 2.
Group 17 elements have the most protons.
Because of the proton pull they would create the
smallest atoms even with added electrons
Using the periodic table trends,
explain why aluminum (Al) is a
better choice than magnesium
(Mg) or Iron (Fe) for certain
real world uses such as boats
and house siding.
112
Aluminum would be less reactive
than magnesium and iron since it is a
metal located to the right of
magnesium and iron on the periodic
table. So, it won’t undergo chemical
change as readily as magnesium or
iron would.
113
What 2 major problems did
Mendeleev have when he
constructed his Periodic Table?
114
Final Answer
Some elements hadn’t yet been
discovered yet
Some elements did not “fit”
according to their atomic mass
115
A seat of honor at
the Periodic Table
JK: + 3 points!
116