Topic 1 Flashcards

1
Q

Trend down group 7

A

-7 electrons on outer shell
-electronic configuration determine reactivity

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2
Q

Arrows in orbitals

A

Have the same spin
(ignore rotate in same direction)

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3
Q

Reactivity of barium and strontium

A

-sum of ionisation energy for barium is lower so barium is more reactivity
-barium is bigger
-barium has more shielding and bigger distance
-bigger nuclear charge
-shielding outweighs nuclear charge so barium is more reactive

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4
Q

Deductions made from ionisation energy graph

A

-jump between -and - electron removed
-group number
-configuration (in terms of shells, ex 2,8,1)

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5
Q

How many electrons are there in 3rd subshell

A

18

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6
Q

Mass spectra

A

-compare no. of each isotope detected
-through mass spectrometer
-magnetic field (NOT electric)

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7
Q

Why should mass spectrometry be in a vacuum

A

to prevent collisions with air molecules

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8
Q

Polarisation

A

-molecule distorted and not spherical
-higher charge and smaller radius
-orbitals overlap and electrons move towards
-not fully separate though

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9
Q

Why is potassium ion smaller than potassium atom

A

-one less shell
-electrons held more tightly as same number of protons attract less electrons

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10
Q

Define orbital

A

A region where electrons are highly likely to be found

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11
Q

Difference in ionisation energy in calcium

A

2-3-third electron lost is from a subshell closer to the nucleus so more attraction
1-2-small change as they are from the same subshell

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12
Q

Periodicity

A

-repeating trend
-atomic radius decrease across period
-repeated in group 3,4,5…

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13
Q

Scandium and zinc

A
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14
Q
A
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