Atomic Structure and the PT

Question 1

Relative isotopic mass def

Answer 1

The mass of an atom of an isotope divided by 1/12 the mass of a carbon-12 atom

Question 2

How do you work out molecular mass and molar mass?

Answer 2

Find the relative formula mass by adding up all the atomic masses of all the elements in the formula. Then put units of grams on the end

Question 3

Equations involving mass, amount and Mr

Answer 3

n= m/Mr
Mr= m/n
m= n x Mr

n - amount (mol)
m - mass (g)
Mr - relative formula mass (no units)

Question 4

Equations involving molar gas volume, volume of gas and moles of gas

Answer 4

volume of gas = 24 x moles of gas

moles of gas = volume of gas / 24

Question 5

Relative molecular mass

Answer 5

The average mass of a molecule relative to 1/12th the mass of an atom of carbon-12

Question 6

Quantum shells

Answer 6

Electron shells. Specify the energy level of an electron

Question 7

Phosphate ion

Answer 7

PO4^3-

Question 8

Describe the relative energies of s-orbitals and p-orbitals

Answer 8

P-orbitals have greater energy than s-orbitals. P-orbitals have equal energies.

Question 9

Orbital def

Answer 9

A region within an atom that can hold up to two electrons with opposite spins

Question 10

Ionisation energy

Answer 10

The energy required to remove one electron from each atom from one mole of gaseous atoms to form one mole of gaseous ions

Question 11

What to remember when writing ionisation energy equations

Answer 11

All need to be in gaseous states. If it’s the third IE (for example), start with the 2+ charge then end with the 3+ charge and an electron

Question 12

How many electrons can orbitals hold

Answer 12

2

Question 13

1s^2 means…

Answer 13

1 =  shell number
s = type of orbital
^2 = number of electrons in shell