CHM-2-Electronic Structure & Periodic Table

Question 1

What are the charges of an:
Electron
Proton
Neutron

Answer 1

-1
+1
0

Question 2

Ionisation of an atom will make it become an…

Answer 2

Ion - Either a Cation (Positive) or anion (Negative)

Question 3

What are valence electrons? (3 Points)

Answer 3

The electrons furthest from the nucleus of an atom

• Responisble for chemical properties
• Instrumental in chemical bonding

Question 4

What is an isotope? (2 Points)

Answer 4

An element with an unequal number of neutrons to the proton number.
Same atomic number but different atomic mass.

Question 5

What is the ‘dual nature of matter’?

Answer 5

The theory that electrons and subatomic particles are waves as well as particles.

Question 6

What is the Schrödinger equation?

Answer 6

Describes atomic orbitals as complicated wave functions.

Question 7

What are quantum numbers used for?

Answer 7

To describe the theoretical position and therefore energy of an electron.

Question 8

What are the four quantum numbers?

Answer 8

n
ℓ
m\/ℓ
m\/s

Question 9

Quantum number n (3 Points)

Answer 9

The principle quantum number which determines the radial distribution.
-Integer values 1, 2, 3, 4, 5 etc. represent the shell number and orbital size.
-Higher the value of n, the higher the energy
E.g n=1, n=2, n=3

Question 10

Quantum number - ℓ

Answer 10

The Angular Momentum (Azimuthal) quantum number
-Defines the atomic orbital shape
-Takes all integer values between 0 and n -1
E.g n=4 Therefore ℓ=0/1/2/3 (Not 4)

Question 11

Quantum number - m\/ℓ

Answer 11

The Magnetic Quantum Number

• Defines orientation of an orbital
• Can have a value of -1, 0 or 1

Question 12

Quantum number - m\/s

Answer 12

The Spin Quantum Number

• Simply represents the rotational direction of an electron.
• Can have a value of +1/2 or -1/2 (Antiparalell Spins)

Question 13

What shape are orbitals with ℓ = 0?

Answer 13

s-shaped (Sperical) - Angular distribution that is uniform at every angle

Question 14

What shape are orbitals with ℓ = 1?

Answer 14

p-shaped (2 lobes / Dumbell Shaped)

Question 15

What shape are orbitals with ℓ = 2?

Answer 15

d-shaped (4-leafed Clover shaped)

Question 16

What shape are orbitals with ℓ = 3?

Answer 16

f-shaped

Question 17

What shape are p orbitals?

Answer 17

2 lobes / ‘Dumbell’

Question 18

What comes after f-shaped orbitals?

Answer 18

g, h, I, j etc.

Question 19

What is heisenberg’s uncertainty principle?

Answer 19

You cannot know the exact position and speed of an object E.g An electron in orbit.

Question 20

When do values of ℓ = 4 and above occur?

Answer 20

When n ≥ 4.

Question 21

What is Pauli’s exclusion principle?

Answer 21

No two electrons in an atom can have the same four quantum numbers.

Question 22

What is Hund’s rule?

Answer 22

Electrons fill orbitals singly first until all orbitals of the same energy are filled.

Question 23

What is the ground state of an atom?

Answer 23

When the atom is in it’s lowest overall state of energy.

Question 24

What occurs when the atom is in it’s ground state?

Answer 24

Electronic configuration - where electrons fill orbitals in a set order.

Question 25

For a given m\/ℓ, a maximum of ... electrons are allowed.

Answer 25

2

Question 26

"Always fill the lowest energy (ground state) orbitals first"

Answer 26

Aufbau Principle.

Question 27

``` How many orbitals do s-shapes p-shapes d-shapes f-shapes have? ```

Answer 27

1 3 5 7

Question 28

A paramagnetic material is composed of...

Answer 28

atoms with unpaired electrons.

Question 29

A paramagnetic material is ........ a magnetic field.

Answer 29

Attracted to

Question 30

A diamagnetic material is composed of...

Answer 30

atoms with paired electrons

Question 31

A diamagnetic material is ........ a magnetic field.

Answer 31

Repelled by

Question 32

What is the strongest form of magnetism?

Answer 32

Ferromagnetic magnetism

Question 33

The excited state configuration is when...

Answer 33

Electrons are promoted to higher unoccupied/partially occupied orbitals through energy input into the electron.

Question 34

The 'n' value is equal to...

Answer 34

The row or period number on the periodic table.

Question 35

When an orbital is one electron from being half full or full, what occurs?

Answer 35

An electron from the lower subshel jumps to make the next subshell more stable.

Question 36

In metal ions, transition energies from d-electrons can casue...

Answer 36

coloured solutions

Question 37

What is the first Ionisation energy/potenital (IE/IP)?

Answer 37

The energy required to remove one of the outermost valence electrons from an atom in it's gaseous state.

Question 38

First IE/IP increases as...

Answer 38

You move from left to right accross a period | You move from the bottom to the top of a group

Question 39

What is the second ionisation energy/potential (IE/IP)

Answer 39

The energy required to remove a second valence electron from the ion to form a divalent ion.

Question 40

What is electron affinity (EA)?

Answer 40

The energy change that acompanied the following process: X(g) + 1e- ->X-(g) (X is a given element)

Question 41

What can the electron affinity be used to measure?

Answer 41

The ability of an atom to accept an electron - The stronger the attraction of a nucleus, the greater the electron affinity.

Question 42

Why do halogen atoms have a very negative EA?

Answer 42

Because they have a great tendancy to form negative ions.

Question 43

Element's EA become more negative as...

Answer 43

You move from left to right on the periodic table | Do not change going down columns

Question 44

From left to right, the atomic radius of elements

Answer 44

Decrease

Question 45

What is Electronegativity?

Answer 45

Parameter that measures the atom's ability to pull or repel bond electrons.

Question 46

What is determined to achieve the electronegativity value?

Answer 46

1st IE and the EA

Question 47

The greater the value of electronegativity...

Answer 47

the greater it's attraction for bonding electrons

Question 48

The larger the atom... | Electronegativity

Answer 48

The less ability for it to attract electrons for itself in chemical bonding.

Question 49

The lower the difference between electronegativity in two covalently bonded atoms...

Answer 49

The stronger the bond. | -Due to the bond being shared more equally and thus being more stable.

Question 50

Why are metals good conductors?

Answer 50

Their valence electrons can move freely

Question 51

Nonmetals have higher....

Answer 51

Electronegativity and ionisation energies

Question 52

General characteristics of Metals

Answer 52

Hard/Shiny 3 or less valency electrons Form + ions by losing e- Good conductors

Question 53

General characteristrics of Metalloids

Answer 53

Varied appearejce 3-7 valence electrons form + and - ions

Question 54

General characteristics of Nonmetals

Answer 54

Gases/Brittle, dull solids 5+ valence electrons Form - ions by gaining e-

Question 55

Group IA

Answer 55

Alkali Metals

Question 56

Group IIA

Answer 56

Alkaline Earth Metals

Question 57

Group VIIA

Answer 57

Halogens

Question 58

Group 0

Answer 58

Noble gases

Question 59

Which groups are the transition elements?

Answer 59

IB to VIIIB