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A Level Chemistry Ocr > Module 2 Chapter 5 > Flashcards

Module 2 Chapter 5 Flashcards

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1
Q

What happens as the shell number increases

A

The more electrons can be contained in the shell

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2
Q

What happens in terms of energy as the shell number increases

A

As the shell number increases the energy of the shells also increases

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3
Q

Why does the energy of the shells increase as the shell number increases

A

More energy is required to keep them in the atom as they are further away from the nucleus

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4
Q

What is another name for the shell number or energy level number

A

Principal quantum number

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5
Q

What can the maximum number of electrons in each shell be calculated by

A

2N squared (where n is the principal quantum number)

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6
Q

What are the maximum number of electrons in each shell

A

N = 1, maximum number 2
N = 2, maximum number 8
N = 3, maximum number 18
N = 4, maximum number 32

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7
Q

What do electrons behave like

A

Electrons have wave particle duality meaning they behave both as a wave and a particle

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8
Q

What are shells made up of

A

They are made up of atomic orbitals

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9
Q

What can orbitals hold

A

They are a region around the nucleus that can hold up to 2 electrons with 2 opposite spins.

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10
Q

What is an orbital

A

It’s visualised as a region in space where there is a high probability of finding an electron.

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11
Q

What is a property of the electrons in the orbitals

A

They have either up or down spin. When one electron has up spin the other has down spin.

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12
Q

Without observation what state are electrons in

A

They are in superposition when neither is in up spin or down spin, it is in the spin up and down state.

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13
Q

What are the 4 different orbitals

A

S-, p-, d-, and f- orbitals

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14
Q

What is an s orbital

A

Electron orbital in the shape of a sphere.
They can hold two electrons
Each shell from n=1 contains one s orbital

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15
Q

What happens to the s orbital as the principle quantum number increases

A

the radius of the orbital increases

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16
Q

Draw an s orbital

A
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17
Q

What is a p orbital

A

The orbital is in the shape of a dumbell
Each p orbital contains 2 electrons

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18
Q

What are the three types of p orbitals

A

Px,Pz,Py, where the small letter is the axis that they lie on

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19
Q

What do each of the p orbitals look like

A

Draw it

20
Q

What principle quantum number 1 what is the maximum number of electrons and number of each orbitals

A

2 electrons
1S

21
Q

What principle quantum number 2 what is the maximum number of electrons and number of each orbitals

A

8 electrons
1S, 2S, 2P (2Px, 2Py, 2Pz)

22
Q

What principle quantum number 3 what is the maximum number of electrons and number of each orbitals

A

18 electrons
1S, 2S, 2P (2Px, 2Pz, 2Py), 3S, 3P (3Px, 3Py, 3Pz), 3D

23
Q

What principle quantum number 4 what is the maximum number of electrons and number of each orbitals

A

32 electrons

1S, 2S, 2P (2Px, 2Pz, 2Py), 3S, 3P (3Px, 3Py, 3Pz), 3D, 4S, 4P (4Px, 4Py, 4Pz), 4D, 4F

24
Q

How many d and f orbitals exist in principle quantum number 4

A

5 - d
7 - f

25
Q

What does the average energy in the subshells do as the principle quantum number increases

A

the average energy in the subshells increases as the principle quantum number increases

26
Q

What is the exception to this rule

A

The 4S orbital is lower in energy than 3D orbital

27
Q

How do we fill orbitals

A

We fill orbitals in increasing energy

28
Q

What do you use to represent the spin of an electron

A

You represent the different spins with up and down arrows

29
Q

What is Hund’s rule

A

If there are three electrons in a p subshell, one electron will go into each Px, Py, Pz orbital before doubling up

30
Q

What is Pauli’s exclusion principle

A

An orbital can only hold two electrons and they must have opposite spin

31
Q

What are cations and anions

A

Cations = positive ions = lost electrons
Anions = negative ions = gained electrons

32
Q

When forming ions what occurs

A

the highest energy subshells lose or gain electrons

33
Q

How does the exception of 3D and 4S apply to this rule

A

3D is filled last/emptied last
4S is filled first/ emptied first

34
Q

What happens during a chemical reaction between a metal and a non metal

A

The non metal gains electrons forming anions and the metal loses electrons forming cations

35
Q

What is an ionic bond

A

The strong electrostatic forces of attraction between oppositely charged ions.

36
Q

What is the arrangement of ionic structures

A

They are arranged in a giant lattice, and each ion experiences many attractions (as there are ionic bonds in all directions)

37
Q

Why do ionic compounds have a high melting point

A

They are held together by many strong ionic bonds. These take lots of energy to break so ionic compounds have very high melting points.

38
Q

What is the correlation between ion charge and melting point

A

The greater the ion charge the higher the melting point

39
Q

What is the solution lily of ionic compounds

A

Many ionic compounds are soluble in polar solutions. This is because water molecules attract and surround the ions once the lattice is broken.

40
Q

What does the solubility of an ionic compounds depend on

A

It depends on the relative strengths of attraction within the giant ionic lattice structure and the attractions between ions and water molecules.

41
Q

What is the general rule of solubility for ionic compounds

A

Solubility decreases as ionic charge increases

42
Q

What is the electrical conductivity of ionic compounds

A

In the solid state the ions are in fixed positions and are not free to move, they don’t conduct electricity. When liquid or in solution, the charge carrying ions are free to move so conduct electricity.

43
Q

What is a covalent bond

A

The strong electrostatic forces of attraction between a shared pair of electrons and the positive nuclei of the bonded non-metallic elements.

44
Q

What is covalent bonding in terms of 1 bond (orbitals)

A

The overlap between 2 atomic orbitals where each orbital contains 1 electrons, making a shared pair in the overlap

45
Q

What is a double covalent bond

A

The electrostatic forces of attraction between 2 shared pairs of electrons and nuclei of bond atoms

46
Q

What is a triple covalent bond

A

The electrostatic forces of attraction between 3 shared pairs of electrons and nuclei of bond atoms.

47
Q

What is a dative covalent bond

A

The pair of bonding electrons are donated by one of the bonding atoms. You denote this with an arrowhead from the element that provides it.

A Level Chemistry Ocr (8 decks)

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