topic 3 - revision Flashcards

1
Q

chemical vs physical reaction

A

Chemical: rearranges the atoms into the new substances (still made up of the same elements that were present)
Physical: just a different state of the same substance

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2
Q

how do you know if a reaction has occured

A
  • a permanent colour change
  • a gas is given off
  • energy is either produced or absorbed (resulting in a temp change)
  • a precipitate is formed
  • one metal deposits on the surface of another
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3
Q

how is a chemical equation formatted

A

reactants –> products

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4
Q

what is a synthesis/combination reaction

A

where two or more reactants (A and B) combine to produce a single product (AB)

A + B –> AB
Zinc + Oxygen –> Zinc Oxide

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5
Q

what is a decomposition reaction

A

where a compound is broken down into smaller compounds or separate elements (reverse of synthesis)

AB –> A + B
Iron Oxide –> Iron + Oxide

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6
Q

what is a single replacement/displacement reaction

A

where a reactive element (a metal or a non-metal) and a compound react to produce another element and another compound. One of the elements in the compound is replaced by another element

A + BC –> B + AC (where A is metal)
(A is a metal and B is a metal cation and C is an anion)

Aluminium + lead (II) nitrate –> aluminium nitrate + lead

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7
Q

what is a double displacement/precipitation reaction

A

where two ionic solutions react to produce two other ionic compounds. One of the compounds forms a precipitate, which is insoluble. The precipitate floats in the solution the settles and sinks to the bottom.

AB(aq) + CD(aq) –> AD(aq) + CB(s)
AgNO3(aq) + NaCl(aq) –> AgCl(s) + NaNO3(aq)

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8
Q

what are spectator ions

A

the ions not involved in the formation of the precipitate

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9
Q

what is a combustion reaction

A

the rapid reaction of a compound or element with oxygen to form an oxide and produce heat.

hydrocarbon + oxygen –> carbon dioxide + water

CH4 + O2 –> CO2 + H2O

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10
Q

what is a neutralisation or acid rection

A

when an acid reacts with another substance and then they will neutralise each other

acid + bas –> salt + water

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11
Q

what are the reactive metals

A

potassium
sodium
lithium
calcium

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12
Q

what is the law of conservation of mass

A

the law of conservation of mass states that matter cannot be created or destroyed. This means that all atoms present as reactants and products must be in total remain constant

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13
Q

balance Na + Cl2 –> NaCl

A

2Na + Cl2 –> 2NaCl

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14
Q

how does the solid form in a precipitate reaction

A

when the two solutions are mixed, a pos ion and a neg ion combine to form an insoluble compound known as the precipitate.

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15
Q

how do you predict the solid in a precipitate reaction

A

use the solubility table :)

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16
Q

what is enthalpy (H)

A

enthalpy is the stored energy within the chemical bond.

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17
Q

how do you find the change in enthalpy

A

(delta)H = H(products) - H(reactants)

18
Q

what happens during an exothermic reaction

A
  • energy released
  • during the chemical reaction, the bonds are broken and the atoms rearrange to form new chemical bonds
  • temperature in created (delta T = pos)
  • change in enthalpy = neg
19
Q

why is the change in enthalpy negative during an exothermic reaction

A

it is negative because there is less energy being stored and more energy being released into the surroundings

20
Q

what happens during an endothermic

A
  • energy absorbed
  • during the reaction, the reactant bonds are broken and the atoms rearrange to form new chemical bonds
  • temperature decreases (delta T = neg)
  • change in enthalpy = pos
20
Q

why is the change in enthalpy positive in endothermic reactions

A

it is positive because there is more energy being stored and absorbed hence making the change in enthalpy positive

21
Q

what is specific heat capacity

A
  • the amount of heat required to raise the temperature of 1.00g of the substance by 1.00 degrees Celsius
22
Q

what is the formular for specific heat capacity

A

energy (j) = M x C x delta T

23
Q

what is metallic bonding

A

a metallic bond is the force of attraction between cations (metal and metal) and the delocalised electrons in the 3D lattice

24
Q

what is electronegativity

A
  • the ability to hold onto electrons
  • if metals have less than 4 electrons in outer shell it will prefer to lose electrons hence low electronegativity
25
Q

what are the properties of metals and the explanations of them

A
  • malleable; bend into a shape - if a metal has an external force applied the cation and delocalised e’s can move into different shapes
  • ductile; draw into a wire - same reason as malleable
  • conductors of electricity and heat; free moving particles and heat transfers through 3D lattice - valance electrons are not firm within each atom and since the e’s are delocalised that are free to move and carry charge
  • hard/strong/mpt and bpt; not easily broken - metallic bonds are strong
  • lustrous; shiny
  • sonorous; produce sound
26
Q

describe the reactivity of metals

A
  • when a metal is placed into a solution with another metal compound, single displacement reactions may occur
  • in these reactions the 2 metals compete to combine with the non-metal and the more reactive metal will win
27
Q

what is a redox reaction

A
  • it involves the transfer of electrons from one species to the other
  • it involves 2 half equations the reduction and oxidation equations
28
Q

which half equation is the loss of electrons and which is the gain of electrons

A

OIL - oxidation involves loss
oxidation - involves the loss of elections
electrons are on right side of equation

RIG - reduction involves gain
reduction - involves the gain of electrons
electrons are on left side of the equation

29
Q

what reaction is the oxidant in

A

the reduction half equation

30
Q

what reaction is the reductant in

A

the oxidation half equation

31
Q

what is the electrochemical series

A
  • a table of relative oxidation and reduction strengths
  • increase of reduction goes up the left side and increase in strength goes down the right side
32
Q

how do you know a chemical reaction has occurred according to the electrochemical series

A

the oxidant must be higher than the reductant or the line between them must be a negative gradient

33
Q

what are electrochemical cells

A

electrochemical cells are designed to make use of the displacement reactions by separating the two half reaction by making use of the electrical energy produced by the transfer of electrons

34
Q

what is the purpose of the salt bridge in the galvanic cells

A

required to balance the charge changes by providing more ions in each beaker and to complete the circuit

35
Q

what half equation will be the anode

A

oxidation

36
Q

what half equation be the cathode

A

reduction

37
Q

what is the oxidation number of an element in its natural form

A

zero

38
Q

what is the oxidation number of a changed particle

A

what ever the number of the charge is

Al+3 = 3
S-2 = -2

39
Q

oxidation number for hydrogen

A

in non-metal compounds = 1
in metal hydrides = -1

40
Q

oxidation numbers for oxygen

A

normal = -2
peroxide compounds = -1
bonded with fluorine = 2