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Chemistry > paper 1 mock > Flashcards

paper 1 mock Flashcards

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1
Q

How the position of an element in the periodic table is
related to the arrangement of electrons in its atoms and
to its atomic number

A

they are arranged in order of atomic (proton) number

so elements with similar properties are in columns (groups)

electrons in the same group have the same number of electrons in it’s outer shell- this gives them similar chemical properties

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2
Q

what are group 1 elements called

A

alkali metals

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3
Q

what do group 1 elements react and produce (3)

A
  • all react with oxygen to create an oxide
  • all react with chlorine to form white precipitate , metal chloride salts 2NaCl
  • all react with water to produce hydrogen gas and metal hydroxides
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4
Q

how does the reactivity change in group 1 elements

A

reactivity increases- outer electron easily lost

low melting,boiling points

higher relative atomic mass

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5
Q

three characteristics of alkali metals

A
  • all have 1 electron in their outer shell
  • soft and have a low density
  • first three are less dense than water Li,Na,K
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6
Q

• explain how properties of the elements in Group 1 depend on
the outer shell of electrons of the atoms

A

reactivity increases as atoms get larger

the distance between nucleus and outer electrons increases

attraction from the nucleus decreases

allowing them to more easily lose electrons

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7
Q

how do Group 1 elements react with water

A

release hydrogen and form hydroxides

this dissolves too form alkaline solutions

react vigorously with water

fizzing and moving around the surface of water

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8
Q

how do Group 1 elements react with oxygen

A

react with oxygen to create oxide

LI-red flame, white solid
Na-orange flame,white solid
K-lilac flame,make solid immediately

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9
Q

how do Group 1 elements react with chlorine

A

to form white precipitate
Li-white powder
Na-yellow flame, cloudwhite powder
K-more vigorous than sodium

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10
Q

how group 1 metals react with non-metals

A
  • form ionic compounds
  • soluble white solids to form colorless solutions
  • 1 electron in outer shell
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11
Q

what are group 7 elements called

A

Halogens

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12
Q

how properties of the elements in Group 7 depend on

the outer shell of electrons of the atoms

A

-they all have seven electrons in their outer shell

non-metals

exist as molecules with pairs of atoms Cl(2)

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13
Q

characteristics of Group 7 elements (5)

A
  • 7 electrons in outer shell
  • colored vapors
  • diatomic molecules Cl(2)
  • form ionic salts with metals
  • forms molecular compounds with non-metals
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14
Q

group 7 elements their states of matter and colour

A 
Fluorine= pale yellow gas
chlorine= pale green gas
bromine= dark brown liquid
iodine= grey solid, purple vapour
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15
Q

trends in group 7 elements as you go down the group

A

higher relative molecular mass
higher melting and boiling point
less reactive- less easily to gain electrons

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16
Q

What are redox reactions?

A

one substance is reduced and the other substance is oxidised

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17
Q

what do acids and some metals produce

A

acid + metal-> salt +hydrogen

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18
Q

redox reaction of hydrochloric acid and magnesium

2HCl + Mg -> MgCl2 + H2

A
  • Mg -> Mg 2+ + 2e - , Mg has lost electrons so Mg has been oxidised
  • 2H + + 2e - -> H2 , H has gained electrons, so H has been reduced
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19
Q

which metals in the reactivity series will react with acid

A

those above hydrogen

20
Q

general equation for neutralization reaction

A

base + acid-> salt + water

21
Q

general equation between metal carbonate + acid

A

metal carbonate + acid -> salt+water+ carbon dioxide

22
Q

equation for metal oxides + acid

A

metal oxides + acid -> salt+ water

23
Q

how is a soluble salt formed

A
  • react the excess acid with some insoluble chemical (metal oxide)
  • filter off left overs
  • crystallise the product
24
Q

what does acid and alkalis produce in aqueous soloutions

A

acids produce hydrogen ions

alkalis produce hydroxide ions

25
Q

half equations in the extraction of aluminium

A

bauxite Al203 with cryolite
Al 3+ + 3e- –> Al (cathode)

2O2- –> O2 + 4e- (anode)

oxygen reacts with C of the anode producing CO2

26
Q

why is cryolite used in manufacturing of aluminium

A

lowers the melting point of aluminium oxide, reducing energy costs

27
Q

uses of nano particles

A
  • medicine
  • electronics
  • deodorants
  • suncreams, better coverage
28
Q

what is nano science

A

science that studies particles that are 1-100 nm in size

29
Q

why do nano particles have better properties than normal size particles

A

have a higher surface area to volume ratio

30
Q

find the surface area to volume ratio for a cube with a side length of 10 nm

A

each face is 1010=100nm(2)
6 faces so 6100= 600nm(2)

volume of 10cubed= 1000nm(3)

600/1000= 0.6nm(-1)

31
Q

what do atoms contain

A

protins
neutrons
electrons

32
Q

Describe the plum pudding model

A

A ball of positive charge with negative electrons embedded in it

33
Q

describe the Bohr/nuclear model and how it came about

A
  • suggests electrons orbit the nucleus at a specific distance(shells)
  • came from the alpha scattering experiment
34
Q

why the new evidence from the scattering experiment led to a change in the atomic model

A
  • the positively charged alpha particles were being repelled and deflected
  • by a tiny concentration of positive charge in the center of the atom (the nucleus).
35
Q

Difference between the plum pudding model and nuclear model of an atom

A

-in the nuclear model negative electrons are not embedded in it rather orbit the nucleus

36
Q

properties of covalent substances

A

low melting and boiling points (hydrogen and water)

37
Q

what are covalent bonds

A

when non-metal atoms bond together

attracted by electrostatic forces, bonds very strong

38
Q

properties of simple covalent substances

A

-atoms in molecules held together by strong covalent bonds

forces of attraction between molecules very weak

as molecules get bigger the intermolecular forces increases so more energy needed to break bonds

causing melting,boiling points to increase

39
Q

what is an exothermic reaction? give examples

A

energy is transferred to surroundings

so surroundings temperature increases

hand warmers,selfheating can
combustion,oxidation, neutralization

negative sign of energy change

40
Q

what is an endothermic reaction? give examples

A

energy taken in from surroundings

so surroundings temperature decreases

thermal decomposition
sports injury packs

41
Q

what occurs in a chemical reaction in terms of bond energies?

exo/endo, bond breaking/forming

A

exothermic -
energy released from forming bonds is greater than that needed to break bonds

endothermic +
energy needed to break existing bonds is greater than the energy released from forming new bonds

42
Q

what are the advantages (3) and disadvantages (5) of a hydrogen fuel cell

A

+
no pollutants
no recharging
only produces water when burnt

-
flammable
hydrogen difficult to store
fossil fuel production
toxic chemicals
expensive production of hydrogen by electrolysis
43
Q

what are the advantages (2) and disadvantages of rechargeable cells and batteries (2)

A

+
can be recharged by reversing reaction
so fuel doesn’t need to keep being supplied

-
hard to dispose of non-biodegradable
will eventually stop working, need replace

44
Q

what is the overall reaction in a hydrogen fuel cell, what are the half equation?

A

hydrogen goes to anode, oxygen goes to cathode

At the cathode (negative electrode)
2H2 –> 4e(-)+4H(+)

45
Q

what is the overall reaction in a hydrogen fuel cell, At the anode, half equation?

A

oxygen goes to cathode

At the anode (positive electrode)
4H(+) + O2 + 4e(–)→ 2H2O(g)

46
Q

what is the overall reaction in a hydrogen fuel cell,

A

overall=

2H2 + O2 -> 2H2O

Chemistry (14 decks)

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