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IB Chem Periodic Table Unit > Chem Definitions > Flashcards

Chem Definitions Flashcards

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1
Q

Group 1

A

Alkali Metals

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2
Q

Group 2

A

Alkaline Earth Metals

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3
Q

Group 3-12

A

Transition Metals

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4
Q

Group 17

A

Halogens

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5
Q

Group 18

A

Noble Gases/Inert Gases

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6
Q

Metals

A

Left of the staircase

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7
Q

Non-metals

A

Right of Staircase

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8
Q

Outer Electron

A

Determines physical and Chemical properties

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9
Q

Inner Electron

A

Repulsion and Sheilding

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10
Q

Effective nuclear charge experienced by outer electrons is?

A

Less

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11
Q

Across a period the amount of shielding

A

stays the same

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12
Q

Across a period the Nuclear charge

A

increases

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13
Q

Across a period nuclear charge is

A

More effective

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14
Q

Down a Group Effective Nuclear charge

A

Stays the same

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15
Q

Down a Group the nuclear charge

A

Increases by 8

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16
Q

Down a Group shielding

A

Increases by 8

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17
Q

Atomic Radius

A

Half the distance between neighboring atoms

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18
Q

Down a Group Atomic Radius

A

Increases

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19
Q

Why does Atomic Radius increase down a Group?

A

Greater # of PELs

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20
Q

Across a Period Atomic Radius

A

decreases

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21
Q

Why does Atomic Radius increase across a Period?

A

Greater Nuclear Charge, same PEL

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22
Q

Ionic Radius - Cations are

A

smaller than it’s atom

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23
Q

Ionic Radius - Anions are

A

larger than it’s atom

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24
Q

Ionic Radius - Greater Nuclear Charge (+)

A

Smaller ionic radius

25
Q

Ionic Radius -Greater (-) Charge

A

Larger

26
Q

Cation

A

Positively charged ion

27
Q

Anion

A

Negatively charged ion

28
Q

Electron Affinity

A

A measure in the change in energy when 1 mole of electrons are added to 1 mole of gaseous atoms to form gaseous ions

29
Q

X(g) + 1e- => x^-1 (g) shows what?

A

Electron affinity - exothermic

30
Q

Electron affinity is a __________ Process

A

exothermic

31
Q

X-1(g)+1e- => x^-2(g) shows what?

A

Electron Affinity - endothermic

32
Q

Electronegativity

A

A measure of an elements attraction for an electron in a covalent bond

33
Q

What element has the highest electronegativity?

A

Fluorine 4.0

34
Q

What element has the lowest electronegativity?

A

Francium 0.7

35
Q

Down a Group - Electronegativity

A

Decreases

36
Q

Across a Period - Electronegativity

A

Increases

37
Q

Metals - Electronegativity

A

Low

38
Q

Non-metals - Electronegativity

A

High

39
Q

Metals - Melting point trends

A

High, more valence electrons higher melting point

40
Q

Non-Metals - Melting Point Trends

A

Low

41
Q

Metalloids - Melting Point trends

A

Macromolecules, very high melting point

42
Q

Noble Gases - Melting Point Trends

A

Very Low, monatomic

43
Q

Group 1 Alkali Metals lose ___ electron

A

1

44
Q

As you go Down Group 1, reactivity ___________

A

Increases

45
Q

When Group 1 elements react with water they produce _______
solutions

A

Basic

46
Q

Group 1 elements react with group ____ elements to form _________ salts

A

17, ionic

47
Q

The most reactive metal

A

Francium

48
Q

Most reactive non-metal

A

Flourine

49
Q

Metal Oxides are ______

A

Basic

50
Q

Non-metal Oxides are _______

A

Acidic

51
Q

Amphoteric Oxides

A

Can act as both an acid and a base

52
Q

Group 17

A

Halogens

53
Q

Group 17 elements gain ___ electron(s)

A

1

54
Q

Flourine Color

A

Yellow Gas

55
Q

Chlorine Color

A

Yellowish / Green gas

56
Q

Bromine Color

A

Dark Red Liquid

57
Q

Iodine Color

A

Dark Purple

58
Q
A

IB Chem Periodic Table Unit (1 decks)

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