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Chemistry > 9.4 The Periodic Table > Flashcards

9.4 The Periodic Table Flashcards

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1
Q

What is the periodic table? [2]

A

an arrangement of elements in periods and groups in order of increasing atomic number.

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2
Q

What is a physical property? [1]

A

can be observed without changing the identity of the substance - can easily be reversed

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3
Q

What is a chemical property? [1]

A

can only be observed by changing the identity of the substance - cannot very easily be reversed

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4
Q

What are 5 examples of physical properties? [5]

A
  • malleability
  • ductility
  • melting & boiling points
  • odour/ colour
  • state of matter
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5
Q

What are 5 examples of chemical properties? [5]

A
  • pH
  • flammibility
  • reactivity with air/acids/water
  • toxicity
  • ability to corrode
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6
Q

What are valence electrons? [1]

A

the number of outershell electrons

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7
Q

What is valency? [2]

A

the number of electrons its atoms loses, gain or share to form a compound

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8
Q

What is an ion? [2]

A

a charged particle. metals form positive ions (cations); non-metals form negative ions (anions)

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9
Q

What is chemical reactivity based on? [1]

A

electronic configuration

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10
Q

What is a similarity in each group of the periodic table? [1]

A

electronic configurations

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11
Q

What do similar electronic configurations lead to? [1]

A

similar chemical properties

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12
Q

What are 5 physical properties of METALS? [5]

A
  • high melting and boiling point
  • malleable
  • ductile
  • sonorous
  • good conductor
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13
Q

What are 5 physical properties of NON-METALS? [5]

A
  • dull
  • poor conductors
  • brittle
  • not sonorous
  • non-ductile
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14
Q

What are the differences of Group 1 metals compared to other metals? [3]

A
  • soft
  • less dense
  • low melting and boiling points
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15
Q

What is Group 1 called? [1]

A

Alkali metals

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16
Q

Why is Group 1 called Alkali Metals? [2]

A

Group 1 metals are called alkali metals because when reacted it forms an alkali compound - turns purple, pH14

17
Q

What are the general trends going down group 1? [6]

A
  • increase in reactivity
  • increase in atomic radius
  • increase in electron shells shielding the outer electron
  • increase in losing outer shell electron to form a positive ion
  • decrease in melting and boilings points
  • increase in density
18
Q

Why does reactivity increase as you go down group 1? [2]

A
  • shielding is increasing (increased number of shells)
  • less force of attraction
  • distance is greater/ more further apart
19
Q

What is the name given to Group 7? [1]

A

Halogens

20
Q

What is the formula, colour and physical state of Fluorine at rtp? [3]

A
  • F₂
  • orangey-yellow
  • gas
21
Q

What is the formula, colour and physical state of Chlorine at rtp? [3]

A
  • Cl₂
  • yellow
  • gas
22
Q

What is the formula, colour and physical state of Bromine at rtp? [3]

A
  • Br₂
  • red-brown
  • liquid
23
Q

What is the formula, colour and physical state of Iodine at rtp? [3]

A
  • I₂
  • grey
  • solid
24
Q

What are the general trends going down group 7? [7]

A
  • decrease in reactivity
  • increase in atomic radius
  • increase in number of filled electron shells
  • decrease in force of attraction
  • increase is melting and boiling points
  • increase in density
  • colour of element gets darker
25
Q

What are halogen ions called? [1]

A

halides

26
Q

Group 7 are ________ non-metals. [1]

A

diatomic

27
Q

What is the name given to group 8? [1]

A

Noble gases

28
Q

Why are the Noble Gases unreactive? [1]

A

they have a full outer shell

29
Q

Why does reactivity decrease going down group 7? [1]

A

more shielding and distance increases which means it’s harder to attract electrons

30
Q

Group 8 are __________ and __________.

A
  • colourless
  • monoatomic
31
Q

What are the general trends going down group 8? [5]

A
  • increase in density
  • increase in atomic radius
  • increase in number of filled electron shells
  • increase in melting and boiling points
  • ‘potential’ increase in reactivity
32
Q

What is Argon and Helium used for? [2]

A

Argon: fire extinguishers, advertising signs
Helium: filling balloons

33
Q

Transition metals are metals that: [4]

A
  • have high densities
  • have high melting and boiling points
  • form coloured compounds
  • often act as catalysts as elements and in compounds

Chemistry (11 decks)

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