Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chemistry > atomic structure > Flashcards

atomic structure Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

group number

A

number of electrons in outer shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

isotopes

A

atoms same number of protons but different number of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

why do isotopes have same chemical properties

A

same number of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what do periods tell us

A

number of highest energy electron shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

how many electrons does S orbital hold

A

2 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

how many electrons does P orbital hold

A

6 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

how many electrons does the D orbital hold

A

10 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

where do electrons enter first

A

lowest energy orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what happens to atomic radius moving across a period (left to right)

A

decreases

due to increased attraction between nucleus and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

outer shell electrons are… and why

A

partially shielded from attraction of nucleus by electrons in inner shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what happens to atomic radius moving down a group

A

increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

why does the atomic radius increase going down a group

A

less attraction between outer electrons and nucleus

(more shells = further away)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

first ionisation energy

A

minimum energy required to remove one mole of electrons from one mole of gaseous atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

first ionisation energy (definition 2)

A

the enthalpy change when one mole of gaseous atoms forms one mole of gaseous ions with a single positive charge
OR
the enthalpy change of X ➡️ X+➕ e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

why does the atomic radius DECREASE across a PERIOD

A

positive charge in nucleus increases

as number of protons increases
increases attraction between nucleus and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what causes first ionisation energy to increase across a period

A

increased nuclear charge and decrease atomic radius
means outer electrons more attracted to nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

why does boron have a lower first ionisation energy than beryllium

A

2p orbital (boron outer subshell) has higher energy than 2s orbital
takes less energy to remove outer electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

why does ionisation energy increase from carbon to nitrogen but decrease at oxygen

A

each of nitrogen’s electrons are in separate 2p orbitals
oxygen has a pair of electrons in 2p orbital - electrons repel each other = required less energy to remove one of those electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

first ionisation in period 3

A

general increase in first ionisation energy moving across a period (uduuduu)

each of nitrogen’s electrons are in separate orbitals
oxygen has a pair of (2) electrons in orbital - electrons repel each other = required less energy to remove one of those electrons

(looking at third electron shell as its period 3)

20
Q

why does the first ionisation energy decrease going DOWN a GROUP (as well as nuclear charge increasing)

A
  1. atomic radius increases going down group = outer electrons more attracted further from nucleus
  2. number of electron shells increases going down group = more shielding between nucleus and outer electrons
    ↪️ means attraction between nucleus and outer electron decrease going down group
21
Q

whats a successive ionisation energy

A

occurs when further electrons are removed
sequence of ionisation energies

more electrons are removed, each from an ion that is becoming increasingly positive

22
Q

what does a sudden large increase in a graph indicate

A

a change in energy level

23
Q

successive ionisation of oxygen trend

A
  1. increase in IE as we remove first six electrons
    each time outer electron removed
    remaining electrons pulled closer to nucleus
    = greater attraction between electrons and nucleus
    ionisation energy increases
  2. big increase in I.E removing 7th electron
    first 6 e- found in 2nd electron shell,
    7th electron removed from FIRST electron shell
    first electron shell = closer to nucleus (greater attraction)
    electrons in first shell experience less shielding
24
Q

identifying element using ionisation energy (for element in period 3)

A

(work out no. of electrons in outer shell)
1. see gradual increase in ionisation energy (e.g increase from 1st IE to 4th IE = 4 electrons in outer shell = group 4)
2. MASSIVE JUMP = this electron must have been removed from internal shell

group 4 period 3 = Silicon

25
Q

why do atoms react

A

to achieve the electronic configuration of a noble gas

26
Q

formula to find electrons in a shell

A

2n²
where n is the number of the shell
e.g shell 2 = 2(2²)

27
Q

relative charge of proton

A

+1

28
Q

relative charge of neutron

A

0

29
Q

relative charge of electron

A

-1

30
Q

relative mass of proton

A

1

31
Q

relative mass of neutron

A

1

32
Q

relative mass of electron

A

1/1840

33
Q

define relative atomic mass (Ar)

A

the average mass of an atom of an element compared to one twelfth of an atom of carbon-12.

34
Q

relative atomic mass formula

A

average mass of one atom of X ÷ 1/12 x the mass of one carbon-12 atom

35
Q

how are ions formed

A

when an atom loses or gains electrons
no longer neutral and will have an overall charge

36
Q

what is mass spectrometry used for

A

analytical technique used to identify different isotopes and find the overall relative atomic mass of an element

37
Q

steps of mass spectrometry

A
  1. ionisation - electron gun fires high energy electrons at the sample, knocks an electron off (forming a +ve ion)
  2. acceleration - +ve charged ions accelerated towards a -ve charge detection plate
  3. separation - move along a drift chamber, all ions have same K.E so different masses have different velocities
  4. detection - +ve ions hit negative charge detection plate & gain an electron
    size of current ∝ abundance
    ( greater current + greater abundance)
38
Q

what does a plum pudding model show

A

sphere of positive charge with small negative charges distributed evenly

39
Q

what does Rutherfords electron shell model show

A

atom consists of small dense central nucleus surrounded by orbiting electrons in electron shells

40
Q

what is the max amount of electrons that orbitals can hold

A

2 electrons

41
Q

what does the mass number tell us

A

protons and neutrons

42
Q

what does the atomic number tell us

A

protons

43
Q

successive ionisation energy across period 3

A

IE increases across a period
increased nuclear charge
decrease in atomic radius
electron in same energy level
(stronger attraction between nucleus and outer electrons)

44
Q

Deviation 1 aluminium

A

first electron in p-orbital
further from nucleus
higher energy

45
Q

deviation 1 sulfur

A

3ps
Pair of electrons
in the P orbital
rePel each other

46
Q

general trend of period 3

A

number of protons increases
shielding stays the same
increased attraction between nucleus and outer electrons
overall trend = increases

chemistry (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions