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Chemistry > Bohr’s Theory > Flashcards

Bohr’s Theory Flashcards

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1
Q

Lithium Chloride produces the colour

A

Crimson Red

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2
Q

Potassium Chloride produces the colour

A

Lilac

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3
Q

Barium Chloride produces the colour

A

Green

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4
Q

Strontium Chloride produces the colour

A

Dark red

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5
Q

Copper Chloride produces the colour

A

Blue/green

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6
Q

Sodium Chloride produces the colour

A

Yellow

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7
Q

What is an continuous spectrum

A

When white light is passed through a glass prism it produces a array of colours

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8
Q

What is a line emission spectrum

A

a series of coloured lines that correspond to specific frequencies of light emitted when electrons in an element are excited

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9
Q

What is an electron configuration

A

How the electrons are arranged in the shells/energy levels of an atom

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10
Q

Example of emission line spectrum in everyday life

A

Sodium streetlights glow yellow

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11
Q

Describe the flame test

A

Fume cupboard
Concentrated Hydrochloric acid
Platinum wire
If wire is clean there should be no colour produced
Crush salt with Pestle and mortar
Identify the metal from the salt

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12
Q

What is an every level

A

Fixed energy level that an electron in an atom may have

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13
Q

What is the ground state

A

Electrons occupy the lowest available energy level

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14
Q

What is the excited state

A

Where electrons occupy higher energy levels than those available in the ground state

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15
Q

Describe Bohr’s theory

A

Bohr states that electrons reside in fixed energy levels
The hydrogen gaseous ( named substance) electrons are in the ground state
They occupy the lowest energy level and are stable
When and electrical current is passed through the hydrogen gas a fixed amount of this every is absorbed and electrons jump to the next available energy level. Excites state electron are unstable and fall back down to lower levels after a short time and release a photon of light in a definite frequency. Since only definite amounts of energy are emitted, this implies that electrons can occupy only definite energy levels.
Each definite amount of energy emitted gives rise to a line in the emission spectrum.

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16
Q

What is the formula for difference in energy

A

E2-E1 = hf

17
Q

Which is the visible series of energy levels

A

N=2 Balmer series(red visible light)

18
Q

Why do different metals produce different flame colours

A

Each element has a different electron configuration
Therefore different electron transitions are possible
So different frequencies of light will be emitted from each element

19
Q

What does AAS stand for

A

Atomic absorption Spectrometry

20
Q

What is AAS

A

When white light is passed through a gaseous sample of an element, certain wavelengths were missing.
These lines correspond excatly to the lines produced in produced in the emission line spectrum

21
Q

What can AAs be used for

A

Identifying dangerous elements in water

22
Q

List energy sub level from1-4

A

4f
4d
4p
3d
4s
3p
3s
2p
2s
1s

23
Q

What is a Sublevel

A

A subdivision of a main energy level and consists of one or more orbitals of the same energy

24
Q

Who found the wave particle duality

A

Louis de Broglie

25
Q

What is Heisenberg’s uncertainty principle

A

States that it is importable to measure both velocity and position of an electron at the same time

26
Q

Limitations of Bohr’s Theory

A
  1. He didn’t take into account wave particle duality
    2.Heisenbergs uncertainty principle is conflicting
  2. Didn’t take into account sub levels
27
Q

What is an orbital

A

Region in space where there is a high probiotic of finding an electron

28
Q

Who devised a equation to work out the probiotic of finding an electron in a particular sublevel

A

Erwin Schrödinger

29
Q

Describe a S sub level

A

Spherical and each contain 1 orbital

30
Q

Describe a P sub level

A

Dumbbell shaped
Conduits of three orbitals (Px ,Py, Pz)

31
Q

Describe D orbitals

A

They contain 5 orbitals

32
Q

How many electrons does each orbital hold

A

2

33
Q

What is wave particle dualitiy

A

All moving electrons actually move in a wave motion

Chemistry (27 decks)

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