topic 1 - atomic structure

Question 1

trends in ionisation energy across a period

Answer 1

charge increases so more attraction to the nucleus and the electron is being removed from the same subshell

Question 2

how many electrons in the
1-4 quantum shell

Answer 2

2
8
18
32

Question 3

molecular ion peak

Answer 3

peak with the highest m/z ratio in the mass spectrum

Question 4

1st ionisation energy

Answer 4

energy required to remove an electron from each atom in one mole of atoms in a gaseous state

Question 5

what is the ionisation energy

Answer 5

the difference between the energy an electron has in the atom and the energy the electron will have once its is lost

Question 6

ionistion energy equations

Answer 6

Al(g) Al+(g) + e-
Al+(g) Al2+(g) + e-
Al2+(g) Al3+(g) + e-
Al3+(g) Al4+(g) + e-

Question 7

how can electromagnetic radiation be analysed

Answer 7

spectroscope
-mass spectrometre
elements emit the same frequency radiation

Question 8

ionisation energy trend down a group

Answer 8

drecreases (except 3,4)
the amount of protons is increasing and consequently charge but the outermost electron is from a shell further from the nucleus so more shielding from nucleus and this is more influential than the increase charge

Question 9

do succesive ionisation energies increase or decrease
why

Answer 9

increase
as more electrons removed the +ve charge has more of an influence on the remaining electrons
more of a pull to the nucleus
more energy is needed

Question 10

atomic radius trend across period

Answer 10

decreases across a period
sheilding has no effect
charge increases
moves the electrons closer

Question 11

shapes of orbitals

Answer 11

Question 12

no of electrons in
s
p
d
f

Answer 12

2
6
10
14

Question 13

whats ar
(relative atomic mass)

Answer 13

the weighted mean mass of an atom of an element compared to 1/12 of the mass of an atom of carbon-12

Question 14

relative isotopic mass

Answer 14

the mass of an indidual atom of a particular isotope relative to 1/12 of the mass of an atom of carbon 12

Question 15

what makes a transition metal

Answer 15

transition metals form a stable ion with a incomplete d subshell

Question 16

atomic emmison spectrosopy

Answer 16

provides evidence for existance of quantum shell

Question 17

electronic configuration

Answer 17

1s2
2s2
2p6
3s2
3p6
4s2
3d10
4p6 ect
-4s2 goes before 3d10 except in ions
in copper and – you fill the d orbital first but s still comes first

Question 18

isoelectronic

Answer 18

same number of electrons or same electronic structure

Question 19

group same properties explanantion

Answer 19

same amount of electrons in the outershell

Question 20

why is the first ionisation energy of sulpure lower than phosphorus

Answer 20

in sulfur the electron is being removed from a orbital with two electrons so the repulsion is higher meaning the electron is lost easier

Question 21

how can the abundance of two isotopes be found

Answer 21

comparing the intensities from mass spectrometry

Question 22

periodicity

Answer 22

a trend of repeating properties with increasing atomic number

Question 23

position of hydrogen above litium p and c

Answer 23

p
-has one outer shell
-forms H+ ions
n
-not an alkali metal
-different chemical properties
-can form H- ions

Question 24

trend in melting temps along period 2

Answer 24

Li to B the bonding is metalic which gets stronger with increased charge as the amount of delocalised electrons increases
Diamond is a giant covalent structure so lots of energy required to overcome the bonds
N to Ne is simple covalent so only weak london forces

Question 25

orbital

Answer 25

region in space where a pair of electrons is likely to be found