Atomic Structure

Question 1

atoms subatomic particles

Answer 1

protons
neutrons
electrons

Question 2

charge of proton

Answer 2

+1

Question 3

mass of a proton

Answer 3

1

Question 4

charge of a neutron

Answer 4

0

Question 5

mass of a neutron

Answer 5

1

Question 6

charge of electron

Answer 6

-1

Question 7

mass of electron

Answer 7

1/1840

Question 8

mass number (A)

Answer 8

sum of protons and neutrons in nucleus

Question 9

atomic number (Z)

Answer 9

number of protons in nucleus

Question 10

isotope

Answer 10

atoms of the same element that have the same number of protons but different number of neutrons

Question 11

relative atomic mass definition

Answer 11

weighted average mass of all isotopes of an atom of an element, relative to 1/12th the mass of an atom of carbon-12

Question 12

relative atomic mass equation

Answer 12

∑(isotopemass × abundance) / totalabundance
​

Question 13

max electrons for an energy levels equation

Answer 13

n = 2n^2

Question 14

orbitals

Answer 14

regions in space where electrons are most likely to be found

Question 15

ionisation energies

Answer 15

energy to remove one mole of electrons from one mole of atoms in its gaseous phase

Question 16

ionisation energy changes across a period

Answer 16

ionisation energy increases across (left to right) a period
due to increasing nuclear charge (more protons but same shielding)
which decreases atomic radii
so attraction between negative electron and positive protons increases
so more energy needed to remove one mole of electrons from one mole of atom in gaseous state

Question 17

ionisation energy changes down group

Answer 17

ionisation energy decreases down group
as atoms get larger
so more shielding (more energy levels)
so weaker attraction between outer electrons and positive nucleus
so less energy is required to remove one mole of electrons form one mole of an atom

Question 18

Pauli exclusions principle (electron spin)

Answer 18

two electrons in same orbitals must have opposite spins (upspin or downspin)

Question 19

hunds rule (electrons in orbitals)

Answer 19

electrons will occupy degenerate orbitals (same energy) singly before pairing up to fill one orbital in order to minimise electron pair repulsion

Question 20

effective nuclear charge

Answer 20

net positive charge experienced by an electron in an atom, considering nuclear charge and sheilding

Question 21

s orbital

Answer 21

spherical orbital
one s orbital in each energy level
max s orbital can hold up to two electrons

Question 22

p orbital

Answer 22

dumbbell shaped
three p orbitals in each energy level
max p orbital can hold up to six electrons (3x2)

Question 23

d orbitals

Answer 23

five d orbitals in each energy level
max 10 electrons (2x5)

Question 24

f orbitals

Answer 24

seven f orbitals in each energy level
max 14 electrons (2x7)

Question 25

what element does the s orbitals start

Answer 25

H = 1s

Question 26

what element does p orbitals start

Answer 26

B = 2p

Question 27

what element does d orbitals start

Answer 27

Sc = 3d

Question 28

what element does f orbital start

Answer 28

La = 4f

Question 29

Aufbau principle

Answer 29

electrons fill orbitals starting from lowest energy level to highest

Question 30

first ionisation energy

Answer 30

energy required to remove one mole of electrons from one mole of atoms in the gas phase