Periodic Table Flashcards

1
Q

Define periodicity

A

trends in periodic table

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2
Q

Periods in a periodic table

A

horizontal row

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3
Q

Define groups in a periodic table

A

vertical columns

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4
Q

Why metals become more reactive going down a group (4)

A

atom bigger as go down

electrons farther from nucleus

electrostatic force of attraction weaker

easier for valence electron to be removed

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5
Q

Define metalloids

A

elements with characteristics of metals and non-metals

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6
Q

Properties of metals (6)

A

large atomic radius

conduct heat/electricity

shiny

malleable

shiny

high melting/boiling point

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7
Q

Properties of non-metals (5)

A

smaller atomic radius

no conduction

low melting/boiling point

brittle

dull

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8
Q

What do elements in the same period have the same of

A

same number of electron shells

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9
Q

Why non-metals less reactive as they go down a group (4)

A

atom bigger as go down

electrons farther from nucleus

weaker electrostatic force of attraction

harder for atom to accept electrons

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10
Q

Define a mole (2)

A

amount of substance

6.02 x 10^23 particles

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11
Q

Avogadro’s constant

A

6.02 x 10^23 particles

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12
Q

Formula for number of moles (2)

A

mass(g)/Mr (relative atomic mass)

concentration(mol/dm^3) x volume (dm^3)

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13
Q

Formula for volume of gas under room pressure/temperature

A

moles x 24dm^3

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14
Q

Volume which a mole of gas occupies in room temperature/pressure

A

24dm^3

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15
Q

Properties of group 1 metals (5)

A

soft to cut

shiny but react with air quickly

relatively low melting/boiling points

relatively low density

reactive

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16
Q

Melting point trend of alkali metals

A

decreases as you go down

17
Q

Density trend of alkali metals

A

density increases as you go down

18
Q

Colour of lithium flame

19
Q

colour of sodium flame

A

orange/yellow

20
Q

colour of potassium flame

21
Q

Alkali metal reaction with air

A

metal + oxygen –> metal oxide

22
Q

Alkali metal reaction with water

A

metal + water –> metal hydroxide + hydrogen

23
Q

Alkali metal reaction with halogen

A

metal + chlorine –> metal chloride

24
Q

How metals react with water (4)

A

react vigorously

produce effervescence

float on surface, moving rapidly

make water alkaline

25
Halogen colours (4)
fluorine - pale-yellow gas chlorine - pale-green gas bromine - red-brown liquid iodine - black, shiny solid
26
Halogen reaction with water
halogen + water --> hydrochloric acid + halogen [ending in ic] acid
27
Colour of chlorine solution (reaction with water)
pale yellow
28
Colour of bromine solution (reaction with water)
orange
29
Colour of iodine solution (reaction with water)
yellow/brown
30
Halogen properties (4)
diatomic colour becomes darker as you go down period density increases as you go down period melting point increases as you go down period
31
Define displacement
more reactive element takes less reactive element's place
32
Properties of noble gases (2)
inert/unreactive monoatomic
33
Properties of transition metals (6)
most have high density high melting points not very reactive forms coloured compounds used as catalysts have more than 1 valence electron in outer shell