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FINISHED > C4.1 > Flashcards

C4.1 Flashcards

1
Q
  1. What do atoms of each element have?
A

-atoms of each element have different proton numbers, as it is the proton number which determines what element it is

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2
Q
  1. What happens when you arrange the elements in order of their proton numbers?
A

-it gives repeating patterns in the properties of elements

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3
Q
  1. What happened to early attempts to find connections between the chemical properties of the elements and their relative atomic mass?
A

-they were dismissed by the scientific community

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4
Q
  1. Who were significant individuals in the history of the development of the Periodic Table?
A
  • Döbereiner
  • Newlands
  • Mendeleev
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5
Q
  1. What were the elements originally arranged by? Why?
A

-relative atomic mass as that was the only thing they could measure

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6
Q
  1. What contribution did Döbereiner have to the development of the Periodic Table?
A

-1828
-triads:
similar chemical properties
middle element of triad had average ram of the other two

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7
Q
  1. What contribution did Newlands have to the development of the Periodic Table?
A
  • 1865
  • arranged in order of ram
  • octaves (each 8th element had similar properties)
  • third row broke down as he didn’t leave gaps
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8
Q
  1. Why was Newlands work criticised?
A
  • groups contained elements that didn’t have similar properties
  • he mixed up metals and non-metals
  • he didn’t leave gaps for undiscovered elements
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9
Q
  1. What contribution did Mendeleev have to the development of the Periodic Table?
A
  • 1869
  • arranged in order of ram
  • left gaps so elements had similar properties in vertical rows
  • gaps left for undiscovered elements
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10
Q
  1. How did Mendeleev use his Periodic Table to predict the existence of unknown elements?
A
  • he left gaps for undiscovered elements

- newly discovered elements fit into gaps= supports his arrangement

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11
Q
  1. What do all the elements in each group have?
A

The elements in a group have similar properties

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12
Q
  1. What is a group of elements?
A

A group of elements is a vertical column in the Periodic Table

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13
Q
  1. What is a period?
A

A period is a row of elements in the Periodic Table

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14
Q
  1. What elements on the periodic table are metal and non-metal?
A

Metals are on the left side of a diagonal line from the bottom of boron to the bottom of astatine, non-metals are on the right

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15
Q
  1. What are Group 1 metals also known as?
A

The alkali metals

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16
Q
  1. Which elements are in group 1? What are their chemical symbols?
A
  • lithium= Li
  • sodium= Na
  • Potassium= L
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17
Q
  1. What is a visible property of group one metals?
A

The alkali metals are shiny when freshly cut but tarnish rapidly in moist air due to reaction with oxygen

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18
Q
  1. What are patterns in Group 1 metals?
A

DOWN THE GROUP

  • more reactive
  • higher density
  • lower melting point
  • lower boiling point
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19
Q
  1. Why does REACTIVITY INCREASE down group 1 metals?
A

-Wants to lose 1 electron to be a full shell

Increased atom size= outer electron further away from nucleus= more easily lost

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20
Q
  1. Why does DENSITY INCREASE down group 1 metals?
A

-Because the atoms are bigger so have more mass

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21
Q
  1. Why does MELTING/BOILING POINT DECREASE down group 1 metals?
A
  • Increased atom size= increase in distance of ions to delocalised electrons= weaker metallic bond (electromagnetic force is more spread out)
22
Q
  1. What is the reaction between lithium and water like?
A
  • floats on water
  • gently fizzes and gives of hydrogen
  • dissolves= lithium hydroxide
23
Q
  1. What is the reaction between sodium and water like?
A
  • floats on water
  • heat= melts= silvery ball
  • hydrogen given off
  • dissolves= sodium hydroxide
24
Q
  1. What is the reaction between potassium and water like?
A
  • floats on water faster
  • heat= melts= silvery ball
  • hydrogen given off, and ignited to as enough energy= lilac flame
  • dissolves= lithium hydroxide
25
Q
  1. What is formed when alkali metals react with water?
A

-an alkaline solution of a hydroxide of the metal with the formula (M)OH [‘metal’ hydroxide]

26
Q
  1. What are examples of this hydroxide solution?
A
  • lithium hydroxide (LiOH)
  • sodium hydroxide (NaOH)
  • potassium hydroxide (KOH)
27
Q
  1. What happens in the reaction between alkali metals and chlorine?
A

alkali metals react vigorously with chlorine to form colourless, crystalline salts with the formula (M)Cl [‘metal’ chloride]

28
Q
  1. What are examples of colourless crystalline salts produced in the reaction between alkali metals and chlorine?
A
  • lithium chloride (LiCl)
  • sodium chloride (NaCl)
  • potassium chloride (KCl)
29
Q
  1. What happens to the reactivity and properties of alkali metals as the group is descended?
A

-more reactive
Wants to lose 1 electron to be a full shell
Increased atom size= outer electron further away from nucleus= more easily lost

30
Q
  1. What are examples to show that the alkali metals become more reactive as the group is descended?
A

-more violent the reaction between an alkali metal and cold water, the more reactive it is

31
Q
  1. What are the hazard symbols?
A

-explosive, toxic, corrosive, oxidizing, and highly flammable

32
Q
  1. What does EXPLOSIVE mean? What is an example?
A
  • can explode

- e.g. some peroxides

33
Q
  1. What does TOXIC mean? What is an example?
A
  • can cause death if swallowed, breathed in, or absorbed through skin
  • e.g. Hydrogen cyanide
34
Q
  1. What does CORROSIVE mean? What is an example?
A
  • attacks and destroys living tissues, like eyes and skin

- e.g. concentrated sulphuric acid

35
Q
  1. What does OXIDISING mean? What is an example?
A
  • provides oxygen so other materials can burn more

- e.g. liquid oxygen

36
Q
  1. What does HIGHLY FLAMMABLE mean? What is an example?
A
  • catches fire easily

- e.g. petrol

37
Q
  1. What are the necessary precautions when working with Group 1 metals and alkalis?
A
  • stored in oil as react vigorously with water
  • fire extinguisher close as reactive and spontaneously combust
  • don’t touch it as can react with sweat= heat and corrosive hydroxide
  • apparatus needs to be dry as reacts with water
  • can’t touch skin or eyes as alkaline solutions are corrosive
38
Q
  1. What are Group 7 metals also known as?
A

The halogens

39
Q
  1. Which elements are in group 7? What are their chemical symbols?
A

Chlorine- Cl2
Bromine- Br2
Iodine- I2

40
Q
  1. What are the states of halogens at room temperature and pressure?
A

Fluorine - gas
Chlorine - Dense gas
Bromine - Volatile liquid
Iodine - Crystalline solid

41
Q
  1. What are the colours of these halogens in their normal physical state at room temperature and as gases?
A

Fluorine - Yellow
Chlorine - green
Bromine - Orange
Iodine - Dark grey (gas= Purple vapour)

42
Q
  1. What are the molecules of halogens?
A

The halogens consist of diatomic molecules

43
Q
  1. What are patterns in Group 7 elements?
A

What happens as you go DOWN the group:
-Become less reactive
Wants to gain 1 electron to be a full shell
Increased atom size= outer electron further away from nucleus= harder to gain
-Have a higher melting/ boiling point
Van der Waals dispersion forces

44
Q
  1. What happens to the reactivity of halogens as you go down the group?
A

-reactivity decreases

45
Q
  1. What are examples that show that reactivity of halogens decreases as you go down the group?
A
  • reactions with alkali metals become less vigorous down the group
  • reactions with iron become less vigorous down the group
  • displacement reactions shows which elements (ones further up) are more reactive than others
46
Q
  1. What happens in the reaction between a halogen and an alkali metal (to show decreasing reactivity down the group)?
A

-halogen + alkali metal (e.g. lithium, sodium, potassium)= salts called metal halides (e.g. sodium chloride, potassium bromide, lithium iodide)

47
Q
  1. What happens in the reaction between a halogen and iron (to show decreasing reactivity down the group)?
A

-halogen + iron= coloured solids called iron halides

48
Q
  1. What happens in displacement reactions with halogen (to show decreasing reactivity down the group)?
A

-more reactive element from compound displaces less reactive element (pushes it out)

49
Q
  1. What are the necessary precautions when working with the halogens?
A
  • don’t get in body as chlorine+ iodine= toxic
  • careful with fluorine as is most reactive
  • avoid contact with skin as liquid bromine is corrosive
  • in fume cupboard as they have poisonous vapours which irritate eyes and lungs
50
Q
  1. What must charges add up to in compounds?
A

0

51
Q
  1. What are examples of halides?
A
  • chlorides
  • bromides
  • iodides

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