7. Trends In The Periodic Table Flashcards

1
Q

Atomic radius def.

A

The atomic radius of an atom is defined as half the distance between two nuclei of atoms of the same element that are joined together by a single covalent bond.

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2
Q

Atomic radius increase and decrease

A

Decrease across a period

Increase down groups

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3
Q

Exception to atomic radius

A

Noble gases; they don’t form covalent bonds

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4
Q

2 reasons why atomic radius increases down groups

A
  • new energy level

- screening effect of inner electrons

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5
Q

2 reasons why atomic radius decreases across periods

A
  • increase effective nuclear charge

- no increase in screening effect

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6
Q

Increase in effective nuclear charge: atomic radius

A
  • no. of protons increases
  • increased pos. pull on outer electrons
  • draws closer to nucleus
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7
Q

No increase in screening effect

A
  • extra electrons SAME energy level
  • no new energy level to add to screening effect
  • and shield outer electrons from pos.charge
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8
Q

First ionization energy

A

First ionization energy of an atom is the minimum energy required to completely remove the most loosely bound electron from a neutral gaseous atom in its ground state.

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9
Q

Formulas for ionization energies

A

X(g) —> X+(g) + e-

X+(g) —> X2+(g) + e-

X2+ (g) ——> X3+(g) + e-

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10
Q

Second ionization energy

A

Second ionization energy is the energy required to remove an electron from an ion with one positive charge in the gaseous state.

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11
Q

Ionization increase and decrease

A

Increase across periods

Decrease down groups

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12
Q

2 reasons ionization increase across:

A
  • Increase effective nuclear charge

- decreasing atomic radius

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13
Q

Increase effective nuclear charge : ionization

A

-no.of protons increasing
-increased pos.attraction
-electrons held more firmly
I.e more energy required to remove them

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14
Q

Decreasing atomic radius : ionization

A

-outermost electrons getting closer
-increased attraction between nucleus and electron
,, more energy required for removal

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15
Q

Increase screening effect : ionization decrease

A

-although nuclear charge increases, pos.force canceled out by corresponding screening effect
-outermost electrons shielded from pos pull.
,, easier, less energy to remove

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16
Q

Why is there exceptions to ionization trend?

A

Any sublevel that is completely filled or half filled has extra stability.
More energy required to break into these stable levels- jump in graph.

17
Q

4 exceptions to ionization

A

Be, N, Mg, P

bean magpie ;

18
Q

Evidence for energy levels from ionization

A
  • second e always harder to remove as it’s taken from a K+ ion
  • sudden large jumps imply we’re breaking into a new energy level w extra stability, closer to nucleus
19
Q

2 reasons why ionization values increase

A

-Pos. Charge on ions increases for each e removed : greater pos. Attraction on remaining electrons
- pos ions becoming smaller as e removed.
e closer to nucleus; increased attraction.

20
Q

Electronegativity increase &decrease

A

Same as ionization.
Increase across,
Decrease down.

21
Q

2 reasons electronegativity increase across

A
  • increase effective nuclear charge

- decreasing atomic radius

22
Q

Increase effective nuclear charge: electronegativity increase

A
  • no.of protons increase

- greater pos.attraction on outermost electrons involved in bonding

23
Q

2 reasons for electronegativity decrease

A
  1. Increase atomic radius

2. Increase screening effect

24
Q

Alkali metals what sort of compounds & why

A

Ionic compounds

  • low ionization energy
  • low electronegativity
25
reason alkali reactivity increases down group
- atomic radius increases - screening effect too - causes ioniz.energy to decrease - outermost electrons more easily lost
26
Alkali metals oxygen reaction notes
- form oxides - stored under oil - lose shiny colour when exposed to air
27
Alkali metals oxygen reaction formula
2K + 1/2 O2 —-> K2O
28
Alkali metal + water.what do they form
Hydroxide +hydrogen gas
29
Alkali metal + water formula
Na +H2O —-> NaOH + 1/2H2
30
Halogens notes
- very reactive: need 1 electron - oxidizing agents (take electrons) - not free in nature - most electronegative
31
Halogens reactivity increas/decrees
Increases UP the group
32
Reason halogen reactivity increase up the group
- most electronegative @top - bc electronegativity decreases down - greater pull on electrons - easier to react to draw in other e & fill outer level
33
Halogens experiment
Cl (g) bubbled through bromide ions solution - cl takes e ; more electronegative - turns bromide into bromine - colorless solution turns red
34
Halogens experiment formula
Cl2 + 2Br- —-> 2Cl- + Br2
35
The same can be seen as in the experiment w halogens in..
Bromine + iodide ions —-> iodine
36
Sentence summing up halogen experiment
The more reactive halogen displaced the less reactive halogen from a solution of its ions.
37
Boilin points halogens : increase or decrease
Increase down the group
38
Reason why boiling point increases down group of halogens
- atomic radius increases - electron clouds bigger - greater chance to form temporary dipoles - stronger van der Waals forces
39
Examples of halogens showing the boiling point :
Fl, Cl: gas Br: liquid Iodine : solid. At room temp