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IB chemistry > Topic 2: Atomic structure > Flashcards

Topic 2: Atomic structure Flashcards

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1
Q

Where are neutrons and protons located?

A

In the nucleus

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2
Q

Where are electrons located?

A

In the electron cloud surrounding the nucleus

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3
Q

Mass of electrons, protons, and neutrons (amu)

A

1/1840, 1, 1

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4
Q

(A/Z)X meaning

A

A= mass number
Z= atomic number
X=element symbol

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5
Q

Isotopes

A

Elements that have the same number of protons but a different number of neutrons

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6
Q

Chemical and physical properties of isotopes are…

A

Chemical properties are the same but physical properties are different

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7
Q

Examples of physical properties

A

Appearance, melting point, boiling point, density, solubility and texture

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8
Q

How are isotopes written?

A

With the mass number and elements symbol only (eg: Cl-35)

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9
Q

Relative atomic mass (Ar)

A

The average mass of an atom of the element, taking into account all its isotopes and their relative abundance

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10
Q

What does a mass spectrometer do?

A

It determines the relative atomic mass of an element from its isotopic composition

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11
Q

Why do isotopes have different physical properties?

A

They have different number of neutrons, meaning they have different densities

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12
Q

Why do isotopes have the same chemical properties?

A

Because isotopes have the same number of electrons, which means they take part in the same chemical reactions

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13
Q

Relationship between deflection and charge to mass ratio

A

The amount of deflection is proportional to the charge to mass ratio (m/z)

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14
Q

Relative abundance

A

The percentage of that isotope that occurs in nature

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15
Q

According to the Bohr model, electrons exist in

A

Energy levels

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16
Q

Atomic orbital

A

represents a region of space where there is a high probability of finding an electron

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17
Q

How to calculate relative atomic mass (Ar)?

A

The sum of the isotopic masses multiplied by their percentage abundances are added together and then divided by 100

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18
Q

The Bohr model

A

According to this model, electrons can only occupy certain energy levels within the atom and can transition between these energy levels by absorbing or emitting exact amounts of energy.

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19
Q

Main energy levels

A

numbers (1,2,3,4)

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20
Q

Sub-levels

A

s/p/d/f

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21
Q

s atomic orbital shape

A

Sphere

22
Q

p atomic orbital shape

A

Dumbbell

23
Q

How many orbitals in p sub-level?

A

3 (px,py,pz)–all at right angles to each other

24
Q

Pauli exclusion principle says..

A

An atomic orbital can hold a maximum of 2 electrons and only if they have opposite spins

25
Q

If energy level is n, what is the number of sub-levels and electrons per energy level?

A

n and 2n^2

26
Q

The Aufbau principle

A

electrons fill atomic orbitals of lowest energy first

27
Q

Write the condensed electron configuration of bromine (Z = 35)

A

[Ar] 4s2 3d10 4p5

28
Q

What are the two exceptions to the Aufbau principle?

A

Chromium (Cr) and Copper (Cu)

29
Q

Write the full electron configurations of Copper and chromium

A

Copper: 1s2 2s2 2p6 3s2 3p6 4s1 3d10
Chromium: 1s2 2s2 2p6 3s2 3p6 4s1 3d5

30
Q

Write the electron configuration for the Ca2+ ion

A

1s2 2s2 2p6 3s2 3p6

31
Q

State the electron configuration of a vanadium atom (Z = 23) and the vanadium(II) ion (V2+).

A

Atom: 1s2 2s2 2p6 3s2 3p6 4s2 3d3
Ion: 1s2 2s2 2p6 3s2 3p6 3d3

32
Q

Hund’s rule

A

electrons fill orbitals in the same sub-level singly, before pairing up

33
Q

Why are line spectra also called ‘rainbow barcodes’?

A

Different elements have different characteristic line spectra and can be used to identify elements.

34
Q

Electromagnetic radiation: what is it and how can it be classified?

A

A type of energy that is all around us and takes many forms, such as radio waves, microwaves, X-rays and gamma-rays. Different types of EM radiation can be classified according to their energy, wavelength or frequency.

35
Q

Wavelength

A

Wavelength (λ) is the distance between two crests in an oscillating wave. It has units of distance (m).

36
Q

frequency

A

The frequency (v) is the number of waves that pass a point in one second. It has the units hertz (Hz) or s-1

37
Q

Energy

A

Energy (E) of electromagnetic radiation depends on its frequency: a higher frequency means higher energy and vice versa. It has units of joules (J).

38
Q

The equation of energy, wavelength and frequency of electromagnetic radiation
What does that say about their relationship?

A

c = vλ

  • frequency and wavelength have an inverse relationship
  • energy and wavelength have an inverse relationship
  • frequency and energy have a direct relationship
39
Q

The relative wavelength, frequency and energy of the infrared (IR) region, the visible region and the ultraviolet (UV) region.

A

IR: low energy, low frequency, long wavelength
Visible: medium energy, medium frequency, medium wavelength
UV: high energy, high frequency, short wavelength

40
Q

What characterizes a continuous spectrum?

A

A continuous spectrum shows all the wavelengths or frequencies of visible light

41
Q

What characterizes an absorption spectrum?

A

Some wavelengths of visible light are missing, shown by black lines on coloured background

42
Q

What characterizes an emission light spectrum?

A

Coloured lines on a black background

43
Q

How are absorption line spectra created? Give an example

A

When electrons absorb energy and transition from lower to higher energy levels.
(eg: transition from n=2 to n=3 absorb energy that correspond to the wavelength of red light, transition from n=2 to n=5 absorb energy that correspond to the wavelength of blue light)

44
Q

At the high-energy (left) end of the spectrum, the lines…

A

converge

45
Q

How are emission line spectra created? Give an example

A

When electrons emit energy and transition from higher to lower energy levels.
(eg: transition from n=3 to n=2 emit energy that correspond to red light, transition from n=5 to n=2 emits energy that correspond to the wavelength of blue light)

46
Q

Equation that shows the relationship between energy and frequency

A

E=hv

where E is energy (in J), h is Planck’s constant (6.63 × 10-34 J s) and v is the frequency (in s-1)

47
Q

Why is the hydrogen emission spectrum in particular studied in detail?

A

It is the simplest emission spectrum because it is only looking at the transition of one electron per atom

48
Q

Electron transitions to the n = 1 energy level emit energy that corresponds to the wavelength or frequency of…

A

ultraviolet (UV) radiation

49
Q

Electron transitions to the n = 2 energy level emit energy that corresponds to the wavelength or frequency of…

A

Visible light

50
Q

Electron transitions to the n = 3 energy level emit energy that corresponds to the wavelength or frequency of…

A

Infrared (IR) radiation

IB chemistry (11 decks)

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