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Science > Chemical Reactions and Dynamics > Flashcards

Chemical Reactions and Dynamics Flashcards

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1
Q

physical vs chemical properties

A
  • physical (alterations to physical properties without changing chemical composition)
  • chemical (change to chemical composition, formation of new substance/s)
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2
Q

Mixtures

A
  • not pure
  • variable composition and properties
  • can be physically separated
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3
Q

2 types of pure substances

A

elements, compounds

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4
Q

observing chemical reactions

A
  • alters the way atoms are bonded together
  • types of atoms and total weight remain the same
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5
Q

signs of chemical change

A
  • original substance disappears
  • change in colour
  • gas is made
  • change from solution to suspension
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6
Q

simple basis of a chemical equation

A

reactant + reactant = product/s

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7
Q

conservation of mass

A

atoms cannot be created or destroyed in chemical changes

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8
Q

exothermic reactions

A

energy released, returns much more energy than the activation energy. reactants have more energy than the products, releasing heat
reactants -> products + heat

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9
Q

endothermic reactions

A

absorb heat energy, require supplied energy
reactants + heat -> products

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10
Q

carbonate

A

compounds containing CO3 and a a metal

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11
Q

combustion

A

exothermic, require oxygen to burn

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12
Q

combustion of carbon-based fuels

A

fuel burns -> atoms in fuel compound combine with oxygen to form an oxide compound

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13
Q

incomplete combustion

A

deficiency of oxygen and fuel isn’t burnt fully

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14
Q

corrosion

A
  • corrosion is a natural electrochemical process that causes materials to deteriorate in chemical reactions with their environments
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15
Q

tendency of ions

A

metals lose electrons (+ charge)
non metals gain electrons (- charge)
- ionic compounds usually soluble in water

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16
Q

polyatomic ions

A

made up of 2 or more bonded atoms in a group with 1+ extra electrons

17
Q

precipitation reaction

A

ions form together into a crystal lattice and tiny solid particles that slowly precipitate to the bottom

18
Q

acids

A
  • ionic compounds that dissolve in water
  • release h+ ions
19
Q

bases

A
  • strong bases (alkalis)
  • compound which dissolves in water and releases hydroxide ions (OH-)
20
Q

neutralisation

A

when an acid is mixed with a base, each destroys that other
- produces neutral water and salt

21
Q

photosynthesis

A

6CO2 + 6 H2O + light -> C6H12O6 +6 O2
carbon dioxide + water +light -> glucose + oxygen

22
Q

cellular respiration

A

C6H12O6 + 6O2 -> 6H2O + 6CO2 + energy (ATP)
glucose + oxygen molecules -> carbon dioxide + water + energy

23
Q

valency

A

combining power of an element
- metals in I, II, III create cations
- nonmetals in V, VI, VII form anions

24
Q

cations vs anions

A

cations (pos charge, lose electrons)
anions (neg charge, gain electrons)

25
Q

naming ionic compounds

A

metal first, end of nonmetal to ide

26
Q

organic compounds

A

based on carbon and hydrogen, often contain oxygen
make up for a vast majority of known compounds

27
Q

synthesis reactions

A

two chemical species combine to produce a single compound
A + B -> AB

28
Q

decomposition reactions

A

a single compound decomposes to produce two or more chemical species
AB -> A + B

29
Q

acids and metal carbonates

A

metal carbonates react with acids to produce salt, water and carbon dioxide gas
Acid +Metal carbonate -> salt + water + carbon dioxide

30
Q

acids and active metals

A

acids react with active metals to produce salt and hydrogen gas

31
Q

precipitation reaction

A

solutions are mixed together to produce an insoluble solid
Solution A + Solution B -> insoluble solid C + solution D

32
Q

complete combustion of hydrocarbons

A

oxygen produces carbon dioxide and water as biproducts
hydrocarbon + oxygen -> carbon dioxide + water

33
Q

fossil fuel combustion

A

hydrocarbons releasing original energy gained from the sun and combustion can be complete or incomplete

34
Q

complete combustion

A

burn hydrocarbons in an excess of air, all carbon to carbon dioxide

35
Q

incomplete combustion

A

hydrocarbon converted to a mixture of water, carbon monoxide and soot

36
Q

aerobic respiration

A

form of oxidation reaction, slower than burning of fossil fuels but is more controlled

37
Q

factors that affect rate of reaction

A
  • occurs through collision theory
    temperature (increases kinetic energy)_
    concentration (increase no. of reactant particles)
    catalysts (lowers activation energy)
    pressure (higher no. of collisions)
    particle size (larger particles = more collision)

Science (6 decks)

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