Week 3 - Periodic Table and Properties

Question 1

What are the four quantum numbers?

Answer 1

1. Principal (n)
2. Angular (l)
3. Magnetic (ml)
4. Spin (ms)

Question 2

What can the values of ms be?

Answer 2

-1/2 or 1/2

Question 3

What do each of the four quantum numbers tell us about the orbital/electron?

Answer 3

n: size of orbital
l: shape of orbital
ml: orientation of orbital
ms: direction of electron momentum

Question 4

Electrons possess what kind of momentum?

Answer 4

Angular (similar to a spinning object)

Question 5

No two electrons can have the same…

Answer 5

four quantum numbers

Question 6

An orbital can have how many electrons?

Answer 6

Max. 2

Question 7

If the nuclear charge is higher, the electron is _____ to remove.

Answer 7

Harder

Question 8

Equation to calculate effective nuclear charge?

Answer 8

Zeff = Z - S
Z is atomic number
S is shielding value

Question 9

Explain what electron shielding is.

Answer 9

Inner electrons ‘shield’ outer electrons from the charge of the nucleus; if electrons are in the same shell they shield one another a small amount and make the electrons easier to remove.

Question 10

Why do 1s electrons shield 2p electrons?

Answer 10

2p orbital is farther from the nucleus than 1s orbital. (note that they do not FULLY shield them)

Question 11

L value trend for penetrating power of electrons in the same shell

Answer 11

s > p > d ≈ f

Question 12

Order of atomic orbitals from lowest to highest energy

Answer 12

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f

Question 13

Afbau Principle

Answer 13

Build up the periodic table (or atoms) by adding one proton at a time to the nucleus and one electron around the nucleus to get the ground state electronic configuration. The electrons sequentially fill the lowest energy orbital available.

Question 14

Describe where the s, p, and d orbitals fall on the periodic table

Answer 14

S is left block (and He)
P is right block
D is middle block

Question 15

Orbitals are more stable when they are…

Answer 15

half-filled or fully filled

Question 16

How to determine valence electrons from electronic configuration?

Answer 16

For main group: electrons in highest n are valence
For transition group: (n)s electrons and (n-1)d electrons are valence

Question 17

Number of valence electrons in periodic table

Answer 17

In main group elements, it increases from 1 to 8

Question 18

Isoelectronic

Answer 18

Same number of electrons

Question 19

Atomic radius is largest where on the periodic table (main group elements)?

Answer 19

Bottom left

Question 20

Ionization energy

Answer 20

The energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions

Question 21

formula for ionization energy (IE); in the same element which IE is larger?

Answer 21

atom (g) → ion+ (g) + e-; IE1 < IE2 < IE3…

Question 22

Where on the periodic table is ionization energy highest?

Answer 22

top right

Question 23

Which elements are the exceptions of the ionization energy trend? Why?

Answer 23

B and Al; they have the first np electrons.
O and S; have a fourth np electron

Question 24

Electron Affinity

Answer 24

The energy change that accompanies the addition of 1 mol of electrons to 1 mol of gaseous atoms or ions

Question 25

Formula for electron affinity

Answer 25

atom (g) + e- → ion- (g) ; ∆E= EA

Question 26

Which elements have high electron affinity?

Answer 26

Halides (second last column)

Question 27

Electronegativity

Answer 27

Ability of an atom in a bond to attract electron density toward itself

Question 28

Atoms that have a high electron affinity…

Answer 28

tend to be very electronegative

Question 29

Where on the periodic table is metallic character the highest?

Answer 29

Bottom left

Question 30

When removing electrons to make a cation, which electrons are removed first?

Answer 30

Highest n; eg. 4s is removed before 3d and so on

Question 31

Paramagnetism vs diamagnetism

Answer 31

Para = contains one or more unpaired electron
Dia = only has paired electrons

Question 32

What happens to ionic size and Zeff when an atom ionizes into a cation?

Answer 32

Size decreases, Zeff increases

Question 33

What happens to ionic size when an atom ionizes into a anion?

Answer 33

Size increases, more e-e repulsion

Question 34

In comparing isoelectronic cations and anions, the ____ will have a larger size.

Answer 34

Anion