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Chemistry Lab Exam > Reaction of Common Metals and Properties of Hydrogen > Flashcards

Reaction of Common Metals and Properties of Hydrogen Flashcards

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1
Q

Group 1 refers to

A

the alkali metals

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2
Q

why are group 1 called alkali metals

A

because their hydroxides (compound with OH) are all soluble in bases (aka they are alkalis)

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3
Q

most important common characteristics of group 1 metals

A

a) single electron in the outermost orbital of their atoms

b)low energy required to detach this electron from the atom (ionization energy(

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4
Q

what is the exception to the group 1 metals

A

hydrogen

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5
Q

why is hydrogen an exception to group 1 metals

A

a) it is a diatomic gas while other elements are metals

b) hydrogen can form an anion (H-) while alkali metals CANNOT

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6
Q

describe the salt-like hydrides made by group 1

A

a) have similar structure to alkali HALIDES (metal and halogen react)

b) EXTREMELY reactive with water

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7
Q

what are the products formed when a salt-like hydride reactions with water (group 1)

A

metal hydroxide and hydrogen has

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8
Q

how can underlying electrons in group 1 metals be removed

A

ONLY with very high energies

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9
Q

what is the oxidation state of alkali metals in their compounds

A

+1

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10
Q

describe motion of electrons when group 1 metals are SOLID

A

electrons are held LOOSELY and they can readily pass from association with on atom to another

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11
Q

do group 1 metals show high or low degree of conductivity

A

high - based on how electrons pass readily from one atom to another when the metals are solid

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12
Q

are the alkali metals the most active of the metals and why or why not

A

yes - because their outer electron is held so loosely

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13
Q

can group 1 metals be easily recognized by a flame test

A

yes

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14
Q

sodium flame test

A

yellow

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15
Q

how can one detect potassium from sodium in a flame test

A

potassium is much MUCH less sensitive than the sodium one, so you have to look through blue glass to cut out the yellow of the sodium light to detect the potassium (if sodium is in high amounts)

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16
Q

group 2 are the

A

alkaline earth metals

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17
Q

what are the elements with 2 valence electrons

A

group 2
(magnesium, calcium, strontium, barium and radium)

group 12
(zinc, cadmium, mercury)

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18
Q

what are common characteristics of group 2 and 12

A

a) group 2 elements have the same core electron configuration as the preceding noble gas

b) group 12 elements have core electrons with EIGHTEEN electrons in the outermost CORE shell

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19
Q

describe beryllium and magnesium compared to the other elements in their group

A

are smaller and have more acidic cations

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20
Q

why were beryllium and magnesium often classified with group 12 elements instead of group 2

A

because of the fundamental differences in their structures (that they are smaller and have more acidic cations)

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21
Q

describe the properties of group 2 hydroxides (EXCLUDING beryllium and magnesium)

A

distinct alkaline properties (basic_

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22
Q

what is the oxidation state of group 2 metals

A

+2

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23
Q

what does group 2 oxidation state mean

A

both their outer electrons are ALWAYS lost when element enters a chemical reaction

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24
Q

describe the ionization energies of the HEAVIER elements of group 2 and 12

A

as low as the alkali metals (reacts more readily with water to lose its electrons)

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25
Q

what happens when group 2 metals react with water

A

form the specific cation (+2), hydroxide (OH-) and hydrogen gas

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26
Q

is the reaction between group 2 metals with water slower or faster than group 1

A

slower

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27
Q

do group 2 metals react with acids

A

YES - very rapidly

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28
Q

how do group 2 metals not undergo rapid oxidation under lower temps

A

because their surfaces are protected by oxide films
- ex. beryllium and magnesium

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29
Q

what are the two of group 2 metals that DO NOT sufficiently impact the flame test

A

beryllium and magnesium

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30
Q

what are some examples of compounds that have a very strong flame test? some that do not?

A

a) chlorides or nitrates

b) oxides or sulfates (due to low volatility)

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31
Q

do zinc and mercury (of group 12) have higher or lower ionization energy than group 2 and why?

A

higher - lack of reactivity of these metals with water

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32
Q

what is the oxidation state of zinc

A

+2

33
Q

how can zinc be easily oxidized

A

with the formation of hydrogen gas (in both acid or basic solutions)

34
Q

what are two examples of amphoteric nature of elements

A

zinc and aluminum

35
Q

what is the compound formed when aluminum reacts with bases

A

Al(OH)4-

36
Q

what of the chemicals used in this lab are extremely dangerous when in contact with moisture

A

sodium and potassium

37
Q

what of the chemicals used in this lab is spontaneously flammable in the air

A

potassium

38
Q

what indicator was used in station 1 (reactions of active metals with water)

A

phenolphthalein as it is colourless in acids or neutral solutions and pink in basic)

39
Q

what metals were used in station 1 of this lab (reactions of active metals with water)

A
  1. sodium
  2. potassium
  3. calcium
  4. magnesium
  5. zinc
40
Q

what was the relative reactivity series of station 1 (reactions of active metals with water)

A

K+ > Na+ > Ca2+ > Mg2+ = Zn2+

41
Q

most reactive alkali metal with water balanced equation

A

2K(s) + 2H2O(l) —-> 2KOH(aq) + H2(g)

42
Q

most reactive alkaline EARTH metal with water balanced equation

A

Ca(s) + 2H2O(l) —-> Ca(OH)2(aq) + H2(g)

43
Q

what happened when sodium was reacted with water

A

immediately reacted and started fizzing and turning into a silver ball before dissolving

b) phenolphthalein turned pink = base present

44
Q

what happened when potassium was reacted with water

A

immediately began to smoke and react with the water

fizzes and dissolves FASTER than sodium

phenolphthalein turned pink = base present

45
Q

what happened when calcium was reacted with water

A

a) immediately sank to the bottom before rising to the surface again

b) it slowly broke apart and some bubbles were observed

c) did react with water but NOT as fast as either potassium or sodium

d) phenolphthalein turned pink = base present

46
Q

what happened when magnesium was reacted with water

A

a) there was NO immediate reaction
b) phenolphthalein = no colour change = acidic or neutral solution

47
Q

what happened when zinc was reacted with water

A

a) immediately sank to the bottom of the water but NO reaction seemed to occur

b) phenolphthalein = no colour change = acidic or neutral solution

48
Q

how to clean up station 1 waste (reactions of active metals with water)

A

a) solutions go down fume hood sink with lots of water

b)metal still in the beaker is thrown in the SOLID CHEIMCAL WASTE BUCKET

49
Q

station 2 of this experiment was

A

flame test of metal ions

50
Q

how to adjust airflow of a bunsen burner

A

turn the tube that connects the end (where flame is) and the base

51
Q

how to adjust gas flow of a bunsen burner

A

by turning the valve (or ring on the base)
- more gas = higher flame
- less gas = lower flame

52
Q

describe the steps of conducting a flame test

A

a) heat a platinum wire in the hottest part of the flame
- if it changes flame colour = clean wire by dipping in 6 M HCl than dipping in RO water before heating again

b) dip the cleaned wire into the solution then heat in the hottest part of the flame

c) clean the wire as in part a and repeat with the next solutions

53
Q

what is the danger with 6 M HCl

A

causes severe burns

54
Q

what were the metals used in station 2 of this experiment (flame test of metal ions)

A

a) calcium

b) Strontium

c) barium

d) lithium

e) sodium

f) potassium

55
Q

of the metals used in station 2 (flame test of metal ions) what were the two flames looked at through didymium glasses

A

sodium and potassium

56
Q

what is the clean up procedure of station 2 (flame test of metal ions)

A

all solutions washed with RO water into the HEAVY METAL WASTE CONTAINER

57
Q

what was station 3 of this experiment

A

reactions of metals with acid and alkali for the identification of hydrogen

58
Q

how was station’s 3 reaction done (reactions of metals with acid and alkali for the identification of hydrogen)

A

a) a spatula-tip full of the metal was added to a large test tube that was filled with 1-2 cm of 6 M HCl

b) the test tube is held with a part of tongs and the reaction is agitated (shaken slightly) to start

c) light a wooden splint over the Tirrill burner and hold it over the opening of the test tube
- do not let splint touch sides of test tube
- use tongs to hold splint AT ALL TIMES

59
Q

what are the two metals used for station 3 (reactions of metals with acid and alkali for the identification of hydrogen)

A

zinc and aluminum

60
Q

the station 3 experiment was conducted twice for each metal, how did the trials 1 and 2 differ

A

a) trial 1 was using 6 M HCl

b) trial 2 was using 10 M NaOH

61
Q

what is a safety note when using NaOH

A

a) it is a strong BASE and can cause burns on skin

62
Q

at station 3, how does on know if hydrogen is present in any of these reactions

A

there will be an audible pop when ignited

63
Q

how is station 3 cleaned up

A

a) all solutions go into the special waste container at the station

b) HCl and NaOH bottles are capped

64
Q

why does hydrogen have a higher first ionization energy than group 1 metals

A
  • electrons are held closer to the nucleus than the group 1 metals
65
Q

why can core electrons of group 1 metals ONLY be removed by high energies

A

they are closer to the nucleus = feel a stronger pull to the nucleus

66
Q

what of the metals used in station 2 was EXPECTED to have the least reaction with water

A

zinc because of its high ionization energy

67
Q

balanced reaction of zinc and hydrochloric acid

A

Zn(s) + 2HCl(aq) —–> ZnCl2 (aq) + H2(g)

68
Q

balanced reaction of zinc and sodium hydroxide

A

Zn(s) + 2NaOH (aq) ——> Na2ZnO2 (aq) + H2(g)

69
Q

balanced reaction of Aluminum and hydrochloric Acid

A

2Al(s) + 6HCl(aq) —–> 2AlCl3(aq) + 3H2(g)

70
Q

balanced reaction of aluminum and sodium hydroxide

A

2Al(s) + 2NaOH (aq)+ 6H2O (l) ——-> 2Na[Al(OH)4] + 3H2(g)

71
Q

describe the reaction of zinc and HCl

A
  • reaction was immediate when zinc was reacted with HCl (bubbles and fizzing)
  • flames burned hotter before the reaction was over
  • a pop is heard which indicates hydrogen is present
72
Q

describe the reaction of zinc and NaOH

A
  • reaction was very slow to start
  • no pop sound was detected = no hydrogen present
73
Q

describe the reaction of aluminum and HCl

A
  • reaction needed heat to start
  • similar reaction was observed to zinc after heating (bubbles and fizzing)
  • no pop was heard = no hydrogen present
74
Q

describe the reaction of aluminum and NaOH

A
  • heat was added to start the reaction
  • a pop can be heard during the reaction with heat
75
Q

calcium flame test colour

A

orange/red flame

76
Q

strontium flame test colour

A

red

77
Q

barium flame test colour

A

green

78
Q

lithium flame test colour

A

red

79
Q

potassium flame test colour

A

violet

Chemistry Lab Exam (4 decks)

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