ATOMIC STRUCTURE

Question 1

Reative mass and charge of proton

Answer 1

1, 1+

Question 2

Relative mass and charge of neutron

Answer 2

1, 0

Question 3

Relative mass and charge of electron

Answer 3

1/1836,1-

Question 4

Behaviour of protons in an electric field

Answer 4

Deflects towards the negative plate

Question 5

Behaviour of neutrons in an electric field

Answer 5

N/A

Because they dont have a charge

Question 6

Behaviour of electrons in an electric field

Answer 6

Deflects towards the positive plate

Greater deflection than protons because electrons have a smaller mass

Question 7

Where is most of an atoms mass concentrated at?

Answer 7

Nucleus

Question 8

Define isotopes

Answer 8

Atoms of the same element with same number of electrons and protons but a different neutron number

Question 9

Define orbital

Answer 9

A region holding upto two electrons w/ opposite spin

Question 10

Describe the shape of an s and a p orbital

Answer 10

s-orbital: spherical
p-orbital: dumb-bell

Question 11

Define a subshell

Answer 11

Division of electron shells into different orbitals

Subshells- s,p,d,f

Question 12

How electrons fill up orbitals?

Answer 12

They fill up the lowest energy orbital available

Question 13

How many orbitals and electrons are present in s, d, & f subshell?

Answer 13

• s: 1 orbital, 2 electrons
• p: 3 orbitals, 6 electrons
• d: 5 orbitals, 10 electons
• f: 7 orbitals, 14 electrons

Question 14

which shubshell orbital has the lowest and highest energy levels?

Answer 14

s has the lowest energy level whilst
d has the highest energy level

Question 15

What subshells are found in shells 1-4?
What is the max no. of electrons that can be found in each shell?

Answer 15

1-s-2
2-s,p-8
3-s,p,d-18
4-s,p,d,f-32

shell-subshell-no. of electrons present

Question 16

what is principal quantum number (n)?

Answer 16

n= the shell that the electron occupies
greater the “n” is the higher the energy is, and farther the shell is from the nucleus.

Question 17

Define first ionisation energy

Answer 17

The energy required to remove an electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions.

Question 18

Is first ionsation of energy exo or endo thermic?

Answer 18

Endothermic

Question 19

Trend in first ionisation energy across period 2 & 3?

Answer 19

As you go along the period, first ionisation energy increases.

Question 20

why does first ionisation energy increase across a period?

Answer 20

• Nuclear charge increases
• Atomic radius decreases
• Shielding remains the same
• Hence electrostatic attraction increases, so more energy is required to overcome these forces to remove an electron from an atom, Ionisation energy therefore increases

Question 21

Trend in first ionisation energy down the group

Answer 21

Ionization energy decreases down the group

Question 22

Why does the first ionisation energy decrease down a group?

Answer 22

nuclear charge increases but-
* atomic radius increases
* shielding increases
* electrostatic attraction decreases, so less energy is needed to overcome these forces to remove an electron from the atom.

atomic radius and shieliding outweigh the nuclear charge

Question 23

Which two elements have an exception and do not follow the electronic configuration pattern?

Answer 23

Chromium
Copper with +2

Question 24

Explain the decrease between beriliyium and boron

across period

Answer 24

Fifth electron of boron is in the 2p subshell, which is further away from the nucleus than the 2s subshell of beryllium

Question 25

Explain the decrease between nitrogen, oxygen and phosphurus

Answer 25

This is due to spin pair repulsion in the 2p orbital of oxygen.