Ionic Radius Trends and Multiple Ionization Energies

Ionic Radius Trends and Multiple Ionization Energies

Presentation

•

Chemistry

•

10th - 12th Grade

•

Medium

•

NGSS

HS-PS1-1, HS-PS1-2, HS-PS1-4

Standards-aligned

Created by

Kristen Vanderveen

Used 403+ times

FREE Resource

20 Slides • 15 Questions

1

Ionic radius trends

Multiple Ionization Energies

Bromfield Honors Chemistry

2

negatively charged ions

form when atoms GAIN electrons

Anions

positively charged ions

form when atoms LOSE electrons

Cations

Ions

Some text here about the topic of discussion

3

negatively charged ions

form when atoms GAIN electrons

Anions

positively charged ions

form when atoms LOSE electrons

Cations

Ions

Some text here about the topic of discussion

4

Ionic radius trends

5

Cations typically have a SMALLER radius than the parent atom

Cations vs parent ion

6

Cations typically have a SMALLER radius than the parent atom

Fewer electrons
Fewer electron:electron repulsions
Fewer occupied energy levels

7

Anions typically have a larger radius than the parent ion

Anions vs parent ion

r

Some text here about the topic of discussion.

8

More electron-electron repulsions

Anions typically have a larger radius than the parent atom

r

9

What is the trend down a group?

What is the trend across a period?

Ionic radius trends

10

Ionic radius increases down a group

Ionic radius trends

11

Ionic radius decreases from L --> R for cations

Jumps up for anions, then decreases

Ionic radius trends

12

Multiple Choice

Which of the following would have the larger radius?

1

Ca

2

Ca²⁺

13

Multiple Choice

Which of the following would have the larger radius?

1

P

2

P^3-

14

Multiple Choice

Which of the following would have the larger radius?

1

Ca²⁺

2

Cl^-

15

Multiple Choice

Which of the following would have the larger radius?

1

K⁺

2

Sc³⁺

16

Multiple Choice

Which of the following would have the larger radius?

1

Cl^-

2

I^-

17

Multiple Choice

Which of the following would have the larger radius?

1

P^3-

2

S^2-

18

Multiple Ionization Energies

19

First ionization energy

The energy required to remove the outermost electron from an isolated gas phase atom

20

Multiple Choice

The equation for the first ionization energy of a sodium atom is:

1

Na (g) + IE ⟶ Na⁺ (g) + e^-

2

Na⁺ (g) + IE ⟶ Na²⁺ (g) + e^-

3

Na⁺ (g) + e^- ⟶ Na (g) + IE

21

Second ionization energy

The energy required to remove a second electron

22

Multiple Choice

The equation for the second ionization energy of a sodium atom is:

1

Na (g) + IE ⟶ Na⁺ (g) + e^-

2

Na⁺ (g) + IE ⟶ Na²⁺ (g) + e^-

3

Na⁺ (g) + e^- ⟶ Na (g) + IE

23

Successive ionization energies

You can have as many ionization energies as there are electrons in the neutral atom
This graph shows the first 7 ionization energies for sodium
As you remove more and more electrons, it takes more and more ionization energy

24

Open Ended

Question image

Why do you think successive ionization energies increase as additional electrons are removed? Hint: Consider electron configurations in your answer.

Type response here

25

Sodium

Consider the values for the first and second ionization energies of sodium

26

Multiple Choice

Question image

When a neutral atom of sodium loses its first electron, the electron is removed from the ____ sublevel.

1

1s

2

2s

3

2p

4

3s

27

Multiple Choice

Question image

When a Na⁺ ion loses an electron, the electron is removed from the ____ sublevel.

1

1s

2

2s

3

2p

4

3s

28

Open Ended

Compare the magnitude of the first and second ionization energies of sodium.

Type response here

29

Removing a second electron from Na

Removing the first electron from Na is relatively easy
To remove a second electron from Na, we have to remove an electron from a noble gas-like electron configuration

30

Removing a second electron from Na

We see a BIG jump in IE values once all the valence electrons have been removed

31

Multiple Choice

Why do we see a big jump in Ionization energy?

1

Because once an element loses all of their electrons there is no more to take

2

Because once an atom loses all their valence electrons, it is harder to take them away

3

Because once the atom becomes an ion it is harder to take electrons away

4

Because once the atom loses 8 electrons it is harder to take them away

32

Successive IE values for Mg

IE₂ > IE₁, as expected
We see a big jump between IE₂ and IE₃

33

Successive IE values for Mg

Removing both electrons from the 3s sublevel is relatively easy
Once we try to remove an electron from a fully filled energy level, it takes a LOT more energy!
This confirms 2 valence electrons for Mg

34

Multiple Choice

Successive ionization energies for an element in Period 4 were found to be:

IE₁=600 kJ/mol

IE₂=1800 kJ/mol

IE₃=2700 kJ/mol

IE₄=11,600 kJ/mol

IE₅=15,000 kJ/mol

How many valence electrons does this element have?

1

1

2

2

3

3

4

4

5

5

35

Multiple Choice

Successive ionization energies for an element in Period 4 were found to be:

IE₁=600 kJ/mol

IE₂=1800 kJ/mol

IE₃=2700 kJ/mol

IE₄=11,600 kJ/mol

IE₅=15,000 kJ/mol.

Identify the element:

1

germanium

2

selenium

3

gallium

4

silicon

5

phosphorous

Ionic radius trends

Multiple Ionization Energies

Bromfield Honors Chemistry

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