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FINISHED > C5.2 > Flashcards

C5.2 Flashcards

1
Q
  1. What is the earth’s hydrosphere?
A

-oceans, seas, lakes and rivers

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2
Q
  1. What does the earth’s hydrosphere consists mainly of?
A

water with some dissolved (ionic) compounds, called salts

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3
Q
  1. How are ions in crystals of a solid ionic compound arranged?
A
  • in a regular way

- forms a lattice

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4
Q
  1. What do solid ionic compounds form?
A

-crystals

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5
Q
  1. How are the ions in a crystal held together?
A

-by forces of attraction between oppositely charged ions

ionic bonding

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6
Q
  1. What are examples of physical properties?
A
  • melting point (turn to liquid)
  • boiling point (turn to gas)
  • electrical conductivity
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7
Q
  1. What is the MELTING POINT of solid ionic compounds like and how does this relate to their bonding and giant, three-dimensional structures?
A

-high
-strong forces of attraction between ions
-need lots of energy to overcome forces
=solid at room temperature

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8
Q
  1. What is the BOILING POINT of solid ionic compounds like and how does this relate to their bonding and giant, three-dimensional structures?
A

-high
-strong forces of attraction between ions
-need lots of energy to overcome forces
=solid at room temperature

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9
Q
  1. What is the ELECTRICAL CONDUCTIVITY of ionic compounds like and how does this relate to their bonding and giant, three-dimensional structures?
A

Can’t conduct electricity normally (solid state)
-has charged particles (ions)
-they are not free to move (to carry charge)
Can conduct when molten or dissolved (in solution)
-charged ions are free to move and carry charge

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10
Q
  1. What happens to the ions when an ionic crystal dissolves in water?
A

-ions separate

=can conduct electricity because charged ions are free to move and carry charge

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11
Q
  1. Why can ionic compounds conduct electricity when dissolved in water?
A
  • ions are charged

- they are able to move around independently in the solution

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12
Q
  1. What are the charges of ions in groups 1,2,3,5,6,7 in the periodic table and why?
A 
1= +1 (lose 1 electron for full shell) 
2= +2 (lose 2 electrons for full shell) 
3= +3 (lose 3 electrons for full shell) 
5= -3 (gain 3 electrons for full shell) 
5= -2 (gain 2 electrons for full shell) 
7= -1 (gain 1 electrons for full shell)
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13
Q
  1. How do you find the formula of salts given their ionic compounds?
A

-swap and drop

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14
Q
  1. What is the formula for the salt sodium chloride (Na-1Cl+1)?
A

-NaCl

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15
Q
  1. What is the formula for the salt magnesium chloride (Mg-2Cl+1)?
A
  • MgCl2
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16
Q
  1. What is the formula for the salt magnesium sulphate (Mg-4SO+1)?
A
  • MgSO4
17
Q
  1. What is the formula for the salt sodium sulphate (Na-4SO+2)?
A
  • Na2SO4
18
Q
  1. What is the formula for the salt potassium chloride (K-1Cl+1)?
A
  • KCl
19
Q
  1. What is the formula for the salt potassium bromide (K-1Br+1)?
A
  • KBr
20
Q
  1. What are examples of salts found in seawater?
A

sodium chloride, magnesium chloride, magnesium sulfate, sodium sulfate, potassium chloride and potassium bromide

21
Q
  1. How can the ions in an ionic compound be detected and identified?
A

-because they have distinct properties and they form compounds with distinct properties

22
Q
  1. How can colours of compounds of metals be used to identify different ions?
A

-flame tests

23
Q
  1. What are the colours of different ions in flame tests?
A
  • sodium= orange/yellow flame
  • potassium= lilac flame
  • calcium= brick red flame
  • copper= blue/ green flame
24
Q
  1. What may occur when mixing two solutions of ionic compounds?
A

-an insoluble compound may precipitate

25
Q
  1. What charge are metal ions?
A

-positive

26
Q
  1. How can some metal (+) ions be identified in solution?
A
  • by adding alkali

- for example sodium hydroxide (NaOH)

27
Q
  1. Why can some metal (+) ions be identified in solution by adding alkali?
A

-because they form insoluble hydroxides with characteristic colours

28
Q
  1. What is a precipitate reaction?
A

-where two solutions react to form an insoluble solid compound called a precipitate

29
Q
  1. What is a precipitate?
A

-an insoluble solid compound

30
Q
  1. What is an example of an alkali that can be used in precipitate reactions?
A

-sodium hydroxide (NaOH)

31
Q
  1. How can some negative ions in salts be identified in solution?
A

-by adding a reagent that reacts with the ions to form an insoluble solid

32
Q
  1. What are examples of a halide?
A
  • chloride
  • bromide
  • iodide

FINISHED (4 decks)

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