Periodic Trends
Presentation
•
Chemistry
•
11th Grade
•
Medium
+1
Standards-aligned
Caleb Grulke
Used 1+ times
FREE Resource
14 Slides • 37 Questions
1
Multiple Choice
2
Multiple Choice
3
Multiple Choice
4
Multiple Choice
Distance and number of protons
Number of neutrons and number of protons
Number of neutrons
and number of electrons
Distance and number of electrons
5
Multiple Choice
Select the element that has the strongest Coulombic attraction.
O
S
Se
Te
6
Multiple Choice
Select the element that has the strongest Coulombic attraction.
O
F
N
C
7
Multiple Choice
Select the element that has the weakest Coulombic attraction.
Fe
Zn
Mn
Sc
8
Ionization Energy
9
10
Multiple Choice
Using the interactive periodic table on the previous slide, what is the trend in ionization energy as you move ACROSS a period on the period table?
Ionization energy INCREASES as you move across
Ionization energy DECREASES as you move across
11
Multiple Choice
Using the interactive periodic table on the previous slide, what is the trend in ionization energy as you move DOWN a group on the period table?
Ionization energy INCREASES as you move DOWN a group.
Ionization energy DECREASES as you move DOWN a group.
12
IONIZATION ENERGY
Ionization energy: the amount of energy required to REMOVE an electron from an atom.
Trend across a period: Ionization energy INCREASES as you move across a period due to INCREASED Coulombic ATTRACTION. Since electrons are more attracted to the nucleus, they are harder to remove/pull away from the nucleus.
13
IONIZATION ENERGY
Ionization energy: the amount of energy required to REMOVE an electron from an atom.
Trend across a Group: Ionization energy DECREASES as you move DOWN a group due to DECREASING Coulombic ATTRACTION. Since electrons are less attracted to the nucleus, they are harder to remove/pull away from the nucleus.
14
Multiple Choice
15
Multiple Choice
Which element has the greater ionization energy?
Magnesium (Mg)
Phosphorus (P)
16
Multiple Choice
Which element has the greater ionization energy?
Iodine (I)
Chlorine (Cl)
17
ELECTRONEGATIVITY
18
ELECTRONEGATIVITY
Electronegativity: Electronegativity is an atom's ability to attract shared electrons in a bond.
Trend across a period: Electronegativity INCREASES as you move ACROSS a period of the periodic table. This is due to INCREASED Coulombic attraction. As electrons are more attracted to an atom's nucleus, it is easier to attract electrons in a bond.
19
ELECTRONEGATIVITY
Electronegativity: Electronegativity is an atom's ability to attract shared electrons in a bond.
Trend across a period: Electronegativity DECREASES as you move DOWN a period of the periodic table. This is due to DECREASED Coulombic attraction. As electrons are more attracted to an atom's nucleus, it is easier to attract electrons in a bond.
20
Multiple Choice
What does electronegativity do as you go across a period?
decrease
no pattern
stay the same
increase
21
Fill in the Blanks
22
Multiple Choice
Why does electronegativity decrease as you go down a group?
As you go down a group, the outer electrons are further away from the nucleus
As you go down a group, the nucleus is less able to attract electrons in a bond
Both of these
None of these
23
Multiple Choice
24
Multiple Choice
The element with the lowest electronegativity in Period 3 is -
Na
Cl
Ar
Mg
25
Multiple Choice
26
ATOMIC RADIUS
27
ATOMIC RADIUS
Atomic Radius: Atomic radius is the distance from the nucleus to the outermost electron.
Trend across a period: Atomic radius DECREASES as you move across a period because of INCREASED Coulombic Attraction. As the attraction increases, electrons are pulled more tightly to the nucleus resulting in a SMALLER radius.
28
ATOMIC RADIUS
Atomic Radius: Atomic radius is the distance from the nucleus to the outermost electron.
Trend down a group: Atomic radius INCREASES as you move down a group because of DECREASED Coulombic Attraction. As the attraction decreases, electrons are allowed to spread out more from the nucleus resulting in a LARGER radius.
29
Multiple Choice
30
Multiple Choice
31
Multiple Choice
32
Multiple Choice
33
Multiple Choice
34
Multiple Choice
35
Multiple Choice
Which element's atom is larger? Nitrogen or Phosphorus?
Nitrogen
Phosphorus
36
Multiple Choice
37
Reorder
Put in order from biggest to smallest (decreasing size)
Calcium
Iron
Zinc
Bromine
Krypton
38
If you want - Label on your periodic table
Note: you don't have to draw the arrows as large as they are on this, but it would be handy to have these labeled as we practice with this.
39
If you want - Label on your periodic table
Note: you don't have to draw the arrows as large as they are on this, but it would be handy to have these labeled as we practice with this.
40
If you want - Label on your periodic table
Note: you don't have to draw the arrows as large as they are on this, but it would be handy to have these labeled as we practice with this.
41
Mixed Practice
42
Multiple Choice
Which atom has the most valence electrons
Ca
C
Cl
Si
43
Multiple Choice
As you move across the periodic table, from left to right, ionization energy is __________________.
decreasing
increasing
44
Multiple Choice
Which atom is more electronegative?
K
Rb
Cl
B
45
Multiple Choice
As you move down the periodic table, atoms tend to get bigger because...
They have more mass
They have more protons
They have more energy levels
They have more mass
46
Multiple Choice
Which statement correctly and completely identifies a trend?
Atomic radius decreases across a period, and increases down a group
Electronegativity decreases across a period and decreases down a group
Ionization energy increases across a period and increases down a group
47
Multiple Choice
Which atom has the largest radius
Mg
B
S
Br
48
Multiple Choice
49
Multiple Choice
50
Multiple Choice
F, N, B
51
Multiple Choice
Show answer
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