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IB Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What is most of the volume of an atom made up of?

A

Electrons (nucleus is very small compared to the total size of the atom)

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2
Q

Where is most of the mass of the atom?

A

In the nucleus

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3
Q

Particle Relative Mass Relative Charge
Proton
Neutron
Electron

A

1 +1
1 0
negligible (5x10^-4) -1

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4
Q

Definition of atomic number (Z)

A

the number of protons in the nucleus of an atom

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5
Q

Definition of mass number (A)

A

the number of protons and neutrons in the nucleus of an atom.

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5
Q

How are positive and negative ions formed? What are they called?

A

+ve loses electron(s) cation
-ve gains electron(s) anion

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5
Q

Calculate % composition of Ir-191 and Ir-193. Atomic mass = 192.22.

A

[191x + 193(100 - x)] / 100 = 192.22
x = 39
Ir-191 = 39%
Ir-193 = 61%

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5
Q

What equipment is used to measure relative abundance of isotopes?

A

Mass spectrometer

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5
Q

Definition of isotope

A

Different atoms of the same element with different mass numbers (numbers of neutrons in the nucleus). Have the same chemical properties (same number of electrons) but different physical properties (melting and boiling points) (different masses so move at different speeds)

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5
Q

Calculate Ar of Li-6 7% and Li-7 93%

A

[(6x7) + (7x93)] / 100 = 6.93

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6
Q

What is the maximum number of electrons in the first five main energy levels?

A

1: 2
2: 8
3: 18
4: 32
5: 50

(2n^2)

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7
Q

state the electromagnetic spectrum and increasing frequency, wavelength, energy.

A

radio wave, microwave, infrared, visible, UV, x-rays, gamma rays

–> increasing frequency
–> increasing energy
<– increasing wavelength

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8
Q

What does a line spectrum for Hydrogen look like?

A

lines get closer at higher frequency. Further away from nucleus, higher energy levels.

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9
Q

What is the difference between a line spectrum and a continuous spectrum?

A

Continuous spectrum: all energies / wavelengths
Line Spectrum: certain energies / wavelengths

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10
Q

How does a spectrum arise? What does this give evidence of?

A

Electron promoted to higher energy level.
Becomes unstable and returns to lower energy level.
Gives out a photon of light, which gives a line in the spectrum.

Electrons being in energy levels – only allowed to have certain amounts of energy.

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11
Q

What level does the electrons fall back to in: UV, visible, Infrared

A

UV: 1
visible: 2
Infrared: 3, 4, 5

12
Q

What region of the Spectrum does the electron fall back to energy level: 1, 2, 3, 4, 5

A

1: UV
2: Visible
3: Infrared
4: Infrared
5: Infrared

13
Q

What is the convergence limit?

A

When the lines merge to form a continuum. The electrons can have any energy and are free from influence of the nucleus (electrons no longer in atom)

14
Q

Give full electron configuration of As

A

1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4^2, 3d^10, 4p^3

15
Q

Give condensed electron configuration of Kr.

A

[Ar] 4s^2, 3d^10, 4p^6

16
Q

What is an orbital?

A

a region of space where there is a high probability of finding an electron (a discrete energy level)

17
Q

How many electrons can an orbital contain?

A

2

18
Q

What does the first shell (in orbitals) contain? What shape is it? Draw it.

A

1s orbital
spherical

19
Q

What does the second shell (in orbitals) contain? What shape are they? Draw them.

A

one 2s orbital, three 2p orbitals
dumb-bell shape – along the lines x, y, z.
degenerate (all the same energy)

20
Q

What does the third shell (in orbitals) contain? Draw them.

A

one 3s, three 3p, five 3d orbitals.

21
Q

What are the number of orbitals in each energy level?

A

s p d f
1: 1
2: 1 3
3: 1 3 5
4: 1 3 5 7
5: 1 3 5 7

22
Q

What is Pauli Exclusion Principle for electrons filling orbitals?

A

The maximum number of electrons in an orbital is two. If there are two electrons in an orbitals they must have opposite spins.

23
Q

What is Hund’s Rule for electrons filling orbitals?

A

Electrons fill orbitals of the same energy (degenerate orbitals) so as to give the maximum number of electrons with parallel spins.

24
Q

What are the electron configurations of 24Cr and 29Cu?

A

[Ar] 3d^5 4s^1
[Ar] 3d^10 4s^1

25
Q

What is the equation for the first ionisation energy for an element?

A

M (g) –> M^+ (g) + e^-

26
Q

What is the equation for the second ionisation energy for an element?

A

Mg^+ (g) –> Mg^2+ (g) + e^-

27
Q

Why is the second ionisation energy always higher than the first?

A

For the 1st IE, and e^- is removed from a neutral atom, but for the 2nd it is removed from a +ve ion. Takes more energy to remove a -vely charged e^- from a +ve ion.

28
Q

Why is the outer electron of potassium easy to remove?

A

it is shielded from the full attractive force of the nucleus by the other shells of electrons.

29
Q

Why is the next electron in potassium considerably more difficult to remove?

A

the electron is in a new shell and is closer to the nucleus and more strongly attracted, and only shielded by ten electrons (electrons in same shell don’t shield each other well) so more strongly attracted.

30
Q

What is the general trend of ionisation energy in elements? Why?

A

increases from left to right across a period.

Electrons added to same shell, but electrons in same shell don’t shield each other well. Force on outer electrons increases from left to right and outer electron is more difficult to remove for neon.

30
Q

Why does Boron have a lower first ionisation energy than beryllium?
Be: 1s^2 2s^2
B: 1s^2 2s^2 2p^1

A

2p sublevel in B is higher in energy than 2s sub level in Be. More energy required to remove e^- from Be.

p e^- in B is shielded to a certain extent by the s electrons so easier to move.

31
Q

Why is the first ionisation energy of oxygen lower than nitrogen?

2p 2p
| | | || | |
N O

A

No p e^- paired in N, less repulsion. 2 e^- paired in same p orbital in O. Electrons repel each other so easier to remove.

32
Q

How does ionisation energy change in a group? Why?

A

decreases down a group.

Smaller atoms higher up. Outer e^- is closer to the nucleus and more strongly attracted, so more energy needed to remove it.

IB Chemistry (6 decks)

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