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CHEMISTRY as - ocr a > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

What are shells

A

Energy levels
Energy increases as shells increase
Shell number = principal quantum number

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2
Q

Atomic orbital

A

A region around the nucleus where there is a high probability of finding an atom
can hold 2 electrons, with opposite spins

S p d f

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3
Q

S orbitals

A

One sphere

Greater the shell number, the greater the radius of the sphere

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4
Q

P orbitals

A

Dumbbell shape
3 orbitals at right angles to each other
X y z

Each shell from n = 2 has 3 p orbitals

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5
Q

D orbitals

A

N=3

5 orbitals

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6
Q

F

A

N=4

7 orbitals

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7
Q

Orbitals fill in order of increasing energy

A

The new type of sub shell added has a higher energy

The highest energy level in the third shell overlaps with the lowest energy level in the 4th shell

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8
Q

Why do electrons pair with opposite spins

A

Electrons are negative and repel each other
They have a property called spin
Electrons in an orbital need to have opposite spins
This helps to counteract the repulsion between the negative charges f the electrons

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9
Q

Electrons in box model rule

A

Fill up each orbital before pairing

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10
Q

Shorthand electron configuration

A

Uses Nobel gas

(He)2s1

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11
Q

Sub shells in periodic table

A

S - 2 groups
P - last 6 groups
D - transition metals
F - below

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12
Q

Ions of d block

A

The energy levels of 4s and 3D are close
Once 3D is filled, it’s energy levels fall below 4s

  • 4s fills and empties before 3D
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13
Q

Wha is ionic bonding

A

The electrostatic attraction between positive and negative ions

Holds cations and anions in ionic compounds

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14
Q

Dot and cross diagrams

A

Outer shell of electrons in metal are transferred to outer shell of non metals to achieve a full outer shell in order to be more stable
Negative and positive ions formed
Has the same structure as the nearest noble gas

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15
Q

Why does a giant ionic lattice form

A

Ions attract oppositely charged ions in all directions

Each ion is surrounded by 6 of the other ion

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16
Q

Properties of ionic lattices

A

Melting points - high
Solubility - in polar solvents
Electrical conductivity - liquid or aqueous solution

17
Q

Melting points of ionic structures

A

Solid at room temperature - insufficient energy to overcome sting electrostatic forces of attraction between opposite charges

A lot of heat needed to overcome this attraction

18
Q

When are melting points higher

A

Lattices with greater ionic charges

Size of ions - bigger they are , more attraction

19
Q

Solubility

A

Ionic compounds dissolve in polar solvents
Polar water breaks down the lattice and surrounds each ion in solution

Lattices with ions of large charges are too strong for water to breakdown - are less soluble

20
Q

Electrical conductivity

A

Solid
Ions are fixed
No mobile charge carriers

Melted / dissolved in water
Solid ionic lattice breaks down
Ions are free to move and carry a charge

Conductor

21
Q

WHat is covalent bonding

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

The overlap of orbitals each containing 1 electron

22
Q

Ions attract in all directions … what about covalent bonds

A

The attraction is localised
Solely between shared electrons and nuclei

Resulting in a molecules - h2 h2o

23
Q

What is a molecule

A

The smallest part of a covalent compound that can exist whilst retaining the chemical properties of a compound

24
Q

Displayed formula

A

Shows the relative positing of atoms and the bonds between them

25
Q

Lone pairs

A

Paired electrons that are not shared

26
Q

Anomalies to covalent dot and cross

A

Boron has 3 outer-shell electrons

Forms boron trifluoride
Has 6 outer-shell electrons

Shows that predictions for bonding can’t be based solely on the noble gas arrangement

27
Q

Phosphorous sulfur chlorine with fluoride

Expansion of the octet

A

N=3 outershell can hold 18 electrons , so more are available for bonding

Only possible when the d shell becomes available for the expansion

28
Q

Double covalent bonds

A

Electrostatic attraction between 2 shared pair of electrons and nucleus

29
Q

Triple covalent bonds

A

Electrostatic force of attraction between 3 shared pairs of electrons and nuclei of binding atoms

N —-N.
H - C —- N

30
Q

Dative covalent bonds

A

A covalent bond in which the shared pair of electrons has been supplied by one of the bonding atoms only

CHEMISTRY as - ocr a (15 decks)

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