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IB Chemistry > 1.3 Electronic Configurations > Flashcards

1.3 Electronic Configurations Flashcards

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1
Q

Highest wavelength

A

radio waves

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2
Q

Lowest wavelength

A

gamma rays

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3
Q

Highest frequency

A

gamma rays

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4
Q

Lowest frequency

A

radio waves

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5
Q

c

A

velocity of wave (3 * 10^8 m/s)

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6
Q

v

A

frequency

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7
Q

λ

A

wavelength

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8
Q

What does a line spectrum show?

A

certain frequencies

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9
Q

When does an electron jump to a higher energy level?

A

when it absorbs energy and increases in energy levels (absorption) (ground to excited state)

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10
Q

When does an electron fall to a lower energy level?

A

when it is unstable and emits a photon to reach a lower energy level (emission) (excited to ground state)

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11
Q

The energy electrons emit is a mix of ____.

A

different frequencies

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12
Q

Packets of energy are called

A

quanta (plural quantum)

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13
Q

Convergence

A

lines get closer towards the blue end of the spectrum

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14
Q

Ionisation energy

A

maximum energy an electron can absorb; any higher causes it to detach from the atom and be ionised

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15
Q

Electromagnetic wave of Lyman series

A

UV

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16
Q

Electromagnetic wave of Balmer series

A

Visible

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17
Q

Electromagnetic wave of Ritz-Paschen series

A

IR

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18
Q

Electromagnetic wave of Brackett series

A

IR

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19
Q

Electromagnetic wave of Pfund series

A

IR

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20
Q

IR series

A

Ritz-Paschen, Brackett, Pfund

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21
Q

Visible series

A

Balmer

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22
Q

UV series

A

Lyman

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23
Q

Dropping from n: ∞ -> 1

A

UV

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24
Q

Dropping from n: ∞ -> 2

A

visible

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25
Q

Dropping from n: ∞ -> 3

A

IR

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26
Q

Dropping from n: ∞ -> 4

A

IR

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27
Q

Arrangement of electrons in an atom is called?

A

electronic configuration

28
Q

Principal quantum numbers describe?

A

energy levels

29
Q

Subshells

A

parts of principal quantum shells

30
Q

Types of orbitals

A

s, p, d, f

31
Q

Subshells contain ____ atomic ____.

A

one or more; orbitals

32
Q

Max number of electrons in an orbital

A

2

33
Q

Shape of s orbital

A

spherical

34
Q

Shape of p orbital

A

dumbbell

35
Q

Shape of d orbital

A

double dumbbell

36
Q

Shape of f orbital

A

irregular

37
Q

Number of orbitals in s subshell

A

1

38
Q

Number of orbitals in p subshell

A

3

39
Q

Number of orbitals in d subshell

A

5

40
Q

Number of orbitals in f subshell

A

7

41
Q

Number of electrons in s subshell

A

2

42
Q

Number of electrons in p subshell

A

6

43
Q

Number of electrons in d subshell

A

10

44
Q

Number of electrons in f subshell

A

14

45
Q

Aufbau principle

A

electrons fill lower energy levels first

46
Q

Electrons always follow a regular pattern in subshells

A

false, irregular after n=3

47
Q

n=1 possible subshells

A

s

48
Q

n=2 possible subshells

A

s, p

49
Q

n=3 possible subshells

A

s, p, d

50
Q

n=4 possible subshells

A

s, p, d,f

51
Q

n=1 max electrons

A

2

52
Q

n=2 max electrons

A

8

53
Q

n=3 max electrons

A

18

54
Q

n=4 max electrons

A

32

55
Q

Difference between 1s and 2s

A

different energy levels (2s orbital is larger than 1s)

56
Q

Format of electronic configuration

A

ns1 (principal quantum number, subshell, electron number)

57
Q

a-block elements have ___ in their a orbital

A

valence electrons

58
Q

Location of s-block elements in the periodic table

A

groups 1 and 2

59
Q

Location of d-block elements in the periodic table

A

transition metals

60
Q

Location of p-block elements in the periodic table

A

metalloids and non-metals

61
Q

Location of f-block elements in the periodic table

A

lanthanides and actinides

62
Q

2 elements that are exceptions to Aufbau principle

A

Cu and Cr

63
Q

Why do exceptions to the aufbau principle exist?

A

the exception configurations are more energetically favorable

64
Q

Full configuration of potassium

A

1s2 2s2 2p6 3s2 3p6 4s1

65
Q

Full configuration of calcium

A

1s2 2s2 2p6 3s2 3sp6 4s2

66
Q

Short configuration of potassium

A

[Ar] 4s1

67
Q

Short configuration of calcium

A

[Ar] 4s2

IB Chemistry (3 decks)

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