Brainscape's Knowledge GenomeTM

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


See full index

IB chemistry > Topic 2: Atomic structure > Flashcards

Topic 2: Atomic structure Flashcards

1
Q

Where are neutrons and protons located?

A

In the nucleus

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

Where are electrons located?

A

In the electron cloud surrounding the nucleus

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

Mass of electrons, protons, and neutrons (amu)

A

1/1840, 1, 1

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

(A/Z)X meaning

A

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

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

Isotopes

A

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

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

Chemical and physical properties of isotopes are…

A

Chemical properties are the same but physical properties are different

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

Examples of physical properties

A

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

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

How are isotopes written?

A

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

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

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

What does a mass spectrometer do?

A

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

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

Why do isotopes have different physical properties?

A

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

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

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

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

Relative abundance

A

The percentage of that isotope that occurs in nature

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

According to the Bohr model, electrons exist in

A

Energy levels

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

Atomic orbital

A

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

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

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

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

Main energy levels

A

numbers (1,2,3,4)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Sub-levels

A

s/p/d/f

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

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