AOS1 Atomic Structure, Periodic Trends and Calculations

Question 1

The Order of subshell filling

Answer 1

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6 ​

Question 2

The Aufbau Principle

Answer 2

states that subshells are filled in order from lowest to highest energy, and that lower energy subshells will be COMPLETELY FILLED before electrons move into a higher-energy subshell.

Question 3

Paulis Exclusion principle

Answer 3

States that only a maximum of two electrons may be found in any given atomic orbital and that if an orbital is filled, the electrons will have opposite spin

Question 4

Hunds rule of max multiplicity

Answer 4

Every orbital in a subshell being singly occupied ( half filled ) BEFORE any orbital in that subshell is doubly occupied ( filled )
in addition, all have filled orbitals have the same spin

Question 5

Definition of Electronegativity

Answer 5

Is the strength with which atoms of an element attract electrons when they are combined with other elements ( think tug of war )

Question 6

Definition of Atomic Radius

Answer 6

Half the distance between two nuclei of a molecule, assuming they are between two identical atoms and a single covalent bond

Question 7

How does the Electronegativity of elements change across a period ( L to R )

Answer 7

It Increases

Question 8

How does the Electronegativity of elements change down a group

Answer 8

It decreases

Question 9

How does the atomic radius of elements change across a period ( L to R )

Answer 9

It decreases

Question 10

How does the atomic radius of elements change down a group

Answer 10

It increases

Question 11

How does the core charge of elements change down a group

Answer 11

It stays constant

Question 12

How does the core charge of elements change across a period ( L to R )

Answer 12

It Increases

Question 13

what is the first ionization energy?

Answer 13

The First ionization energy is defined as the amount of energy required to remove an electron from each of mole of a gaseous atom.

Question 14

Trends of Ionization energy down a group

Answer 14

As you move down a group the first ionisation energy decreases ( required less energy to extract the most valence electron )

Question 15

Trends of Ionization energy across a period ( L to R )

Answer 15

The first ionization energy increases. (more energy requierd to remove an electron)

Question 16

Moles, Mass and Molar mass
What do
n=?
m=?
Mr=?

Answer 16

n=number of mouls
m=mass (in g)
Mr= molar mass

Question 17

One mole of a substance is equal to ( Avogadro constant )

Answer 17

6.022 × 10²³ units of that substance

Question 18

What is N = n x Na

Answer 18

N = number of particles
n = number of moles
Na = Avogadro’s constant ( 6.022 × 10²³ )

Question 19

How do you calclulate for the amount of moles

Answer 19

moles ( n ) = Number of particles/Na

Question 20

what is N = V/Vm

Answer 20

N = moles
v = volume in L
Vm = Molar voulme = 24.8L

Question 21

What is n = CV

Answer 21

n = moles
c = concentration ( mols/L )
v = volume in L