Definitions + Rukes Flashcards

1
Q

Electron orbital

A

Region of space in which an electron spends most of its time

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2
Q

Aufbau principle

A

Electrons fill the lowest available energy level

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3
Q

Hund’s rule

A

Electrons remain impaired in every sub shell as far as possible

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4
Q

1st ionisation energy

A

Energy required to remove 1 electron from each atom in 1 mole of gaseous atoms producing 1 mole of gaseous ions

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5
Q

Linear bond angle

A

180

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6
Q

Tetrahedral bond angle

A

109.5

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7
Q

Trigonal planar bond angle

A

120

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8
Q

Pyramidal bond angle

A

107

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9
Q

Bent bond angle

A

104.5

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10
Q

Octahedral bond angle

A

90

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11
Q

Electronegativity

A

The power of an atom to attract the electrons in a covalent bond

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12
Q

Physical properties of halogens at room temperature

A

Fluorine- pale yellow gas
Chlorine- pale green gas
Bromine- dark red liquid
Iodine- shiny black crystals

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13
Q

KCl + Br2

A

Orange upper layer

Yellow lower layer

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14
Q

KCl and +I2

A

Purple upper layer

Orange lower level

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15
Q

KBr + Cl2

A

Orange upper level

Yellow lower level

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16
Q

KBr+ I2

A

Purple upper layer

Orange lower layer

17
Q

KI+ Cl2

A

Purple upper layer

Orange lower layer

18
Q

Br2+ KI

A

Purple upper layer

Orange lower layer

19
Q

Order of ion tests

A

Carbonates
Sulfates
Halides
Ammonia?

20
Q

Carbonate test

A

Dilute HNO3

Fizzing

21
Q

Sulfates test

A

Excess barium ions eg BaCl2

White precipitate

22
Q

Halide tests

A

Add acidified silver nitrate

Then check with dilute and conc ammonia

23
Q

Ammonia test

A

Add dilute NaOH

When warmed moist ph paper will turn blue

24
Q

Standard enthalpy formation

A

1 mole of substance is formed from its elements in their standard states

25
Enthalpy of combustion
Enthalpy when 1 mole of substance is completely burned in oxygen under standard conditions
26
Enthalpy of reaction
Enthalpy when molar quantities as stated in the chemical equation react together under standard conditions
27
Enthalpy of neutralisation
Enthalpy when and acid and a base react together in their standard stated to form 1 mole H2O under standard conditions
28
Bond enthalpy
The average energy required to break 1 mole of bonds in gaseous molecules
29
Hess’s law
Enthalpy change is independent of the path taken provided initial and final conditions are the same
30
Homogeneous catalyst
Reactants and catalyst in the same state
31
Heterogeneous catalyst
Reactants and catalyst in different states
32
Standard lattice enthalpy
Enthalpy change when 1 mole of an ionic compound is formed from its gaseous ions under standard conditions
33
Enthalpy of atomisation
Enthalpy change when 1 mole of gaseous atoms is formed from the element in its standard state
34
1st electron affinity
Enthalpy change when 1 electron is added to each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1- ions
35
Enthalpy hydration
Enthalpy change when a solutions of ions is made from 1 mole of gaseous ions
36
Enthalpy of solution
Enthalpy change when 1 mole of a solute dissolves to form an infinitely dilute solution
37
Spontaneous reaction
No extra energy is need to continue the reaction