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A Level Chem > A1 - atomic structure, bonding and shapes and molecules > Flashcards

A1 - atomic structure, bonding and shapes and molecules Flashcards

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1
Q

Definition of isotope

A

Atoms of the same element with different number of neutrons and different masses

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2
Q

Definition of isoelectronic

A

Atoms with the same number of electrons

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3
Q

Definition of relative atomic mass

A

The weighted mean mass of an atom of the element compared with 1/12th mass of carbon - 12

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4
Q

Definition of relative isotopic mass

A

The mass of an isotope compared with 1/12th mass of an atom of carbon 12

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5
Q

How many orbitals are in an s-subshell

A

1 - holds two electrons

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6
Q

What is the order of electronic configuration

A

1s2 2s2 2p6 3s2 3p6 4s2 3d10

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7
Q

What is an orbital

A

A region of space where an orbital usually is

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8
Q

Hunds rule about electron configuration

A

Electrons prefer to occupy orbitals on their own and only pair up when no empty orbitals have f the same energy are available

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9
Q

What is the Aufbau principle about electron configuration

A

Electrons are placed into shells starting with the lowest energy level first - each shell must me full before the next shell starts to fill

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10
Q

How many subshells in the first shell

A

1

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11
Q

How many electrons can an s-orbital hold

A

2 electrons

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12
Q

How many electrons can a p orbital hold

A

6

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13
Q

How many electrons can d-orbitals hold

A

10

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14
Q

What orbitals are in the first sub shell

A

S

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15
Q

What orbitals are in the second subshell

A

S and P

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16
Q

What orbitals are in the 3rd subshell

A

S p d

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17
Q

What is the maximum number of electrons in the first shell

A

2

18
Q

What is the maximum number of electron in the 2nd shell

A

8

19
Q

What is the maximum number of electrons in the 3rd shell

A

18

20
Q

Why are 4s subshells filled before 3d subshells

A

4s subshells had lower energy than the 3D subshell

21
Q

Definition of ionic bonds

A

The electrostatic attraction between oppositely charged ions in all directions

22
Q

What two factors determine the strength of ionic bonding

A

Magnitude of charge
Size of ion

23
Q

Why does a smaller ion have a stronger ionic bond

A

More compact electrostatic density so stronger attraction between ions

24
Q

Why does having a larger charge on the ion mean a greater ionic bond

A

Increased pull from the protons in the neutron has a stronger effect on the electrons drawing them closer and having a stronger attraction between ions

25
Q

What is the definition of a covalent bond

A

The electrostatic attraction between a shared pair of electrons and a nuclei

26
Q

Definition of a dative covalent bond

A

Where a shared pair of electrons has come from a single atom

27
Q

What is a sigma bond

A

Bond formed by direct overlap of orbitals

28
Q

What is a pi bond

A

Forms by sideways overlap of p orbitals

29
Q

What shape and bond angle is a molecule with 2 bonded pairs

A

Linear - 180

30
Q

What shape and bond angle is a molecule with three bonded pairs

A

Trigonal planar
120

31
Q

What shape and bond angle is a molecule with 4 bonded pairs

A

Tetrahedral - 109.5

32
Q

What shape and bond angle is a molecule with 5 bonded pairs

A

Trigonal bipyramidal
120,90

33
Q

What shape and bond angle is a molecule with 6 bonded pairs

A

Octahedral - 90

34
Q

Why do bond angles decrease by 2.5 degrees when there are lone pairs

A

Because lone pairs repel stronger than bonded pairs

35
Q

What is the shape and bond angle of a molecule with 3 bonded pairs and 1 lone pair

A

Pyramidal - 107

36
Q

What is the shape and bond angle of a molecule with 2bonded pairs and 2 lone pairs

A

Bent v shape
104.5
109.5-2.5-2.5

37
Q

Definition of relative molecular mass

A

Average mass of a molecule compared to 1/12tb the mass of a carbon atom

38
Q

Definition of Relative atomic mass

A

The average mass of one atom compared to 1/12th the mass of one atom of carbon

39
Q

Electronic configuration of
Cr

A

1s2 2s2 2p6 3s2 3p6 4s1 3p5

40
Q

Cu electronic configuration

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10

41
Q

Why can ice float on water

A

Solid water forms an open lactice where the water particles are spaced further apart making the ice less dense

A Level Chem (8 decks)

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