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chemistry Flashcards

1
Q

what is all matter made of

A

atoms

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2
Q

what is an element

A

a substance made up of one type of atom

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3
Q

how are the elements listed in the periodic table

A

from lowest to highest atomic number

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4
Q

what are the subatomic particles of an atom

A

protons, neutrons, electrons

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5
Q

what subatomic particle(s) are/is in the nucleus

A

protons and neutrons

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6
Q

what charge do protons have

A

positive

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7
Q

what charge do electrons have

A

negative

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8
Q

what charge do neutrons have

A

neutral/no charge

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9
Q

what is the atomic number

A

the amount of protons

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10
Q

what is the mass number

A

the number of protons + neutrons

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11
Q

how is an isotopic symbol laid out

A

mass number on top, atomic number on bottom and chemical symbol next to them

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12
Q

what is the mass of an electron

A

1/1800 of the mass of a proton/neutron

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13
Q

what is the mass of a proton/neutron

A

1800x the mass of an electron, the same as a neutron

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14
Q

how are electrons arranged

A

in shells, in energy levels

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15
Q

what is the equation for the maximum amount of electrons in a shell

A

2n², n is the amount of shells

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16
Q

which shells/electrons have the least energy

A

the closer to the nucleus the less energy the shell/electrons have

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17
Q

how do electrons fill their shells

A

electrons begin to fill shells with lowest energy, closest to the nucleus first

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18
Q

what are periods and how many

A

the horizontal rows, numbered 1 to 7

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19
Q

what are groups and how many

A

groups are vertical rows, numbered 1 to 18

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20
Q

how are ions formed

A

an atom loses or gains electrons to have a full valence shell

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21
Q

why do atoms want a full outer shell

A

to make them stable

22
Q

what is a cation

A

a positively charged ion, loses electron/s usually metals

23
Q

what is an anion

A

a negatively charged ion, gains electron/s usually non metals

24
Q

what happens when an element is heated (flame tests)

A

electrons absorb energy and ‘jump’ to a higher shell (energy level), electron is excited and unstable and releases energy to return to original shell (ground state), this energy is (sometimes) released in form of light

25
what happens to the energy when an electron goes from a higher shell to a lower one
energy is emitted
26
what happens to the energy when an electron goes from a lower shell to a higher one
energy is absorbed
27
how is an isotopic symbol read
top number - mass number bottom number - atomic number superscript - charge of ion
28
what is special about noble gases
they are stable, they have a full outer shell
29
what is ionic bonding
when a non metal and metal react in a chemical reaction and a cation (metal) and an anion (non metal) are formed
30
law of conservation of mass
matter cant be created or destroyed in a chemical reaction, all atoms present at the start are present at the end and the mass of the reactants must equal the mass of the products
31
what happens in a chemical change
a new substance is formed, it is usually difficult to reverse
32
examples of chemical change
burning toast, cooking an egg, baking a cake (baking part), burning wood, rust
33
what does cobalt stand for
colour change, odour, bubbles, appearance/disappearance of a solid, light or sound, temperature change
34
what happens on an atomic level in a chemical reaction
bonds in the reactants are broken, the atoms rearrange and new bonds are formed to make the products
35
what are the symbols in a chemical equation
s - solid aq - aqueous (solution/acid/dissolved) g - gas l - liquid (usually water only)
36
what does the subscript represent (in a word equation)
the number of atoms in a molecule (H₂O has 2 H's and 1 O)
37
what does the coefficient mean (in a word equation)
the number of each molecule and multiplies the subscripts
38
what does a balanced equation need
to represent the law of conservation of mass, needs to have the same amount of each atom in the reactants and products
39
what is the rate of reaction
the speed at which a reaction occurs
40
how is the rate of reaction measured
how fast the reactants are used up or how fast the products are made
41
what must occur for a reaction to take place (particles)
particles of different substances must collide
42
how does collision rate affect reaction rate
the more (successful) collisions in a given time, the faster the reaction
43
what makes a collision successful
molecules collide with enough energy and have the correct orientation (face each other)
44
what happens to the rate of reaction over time
the rate decreases, the concentration of reactants decreases, reducing the frequency of collisions
45
how can the rate of reaction be increased
increase temperature, increase concentration of dissolved reactants, increase surface area of solid reactants and/or use a catalyst
46
how does temperature affect the reaction rate
higher temperatures cause particles to move faster, they have more energy and are more likely to collide with enough energy, number of successful collisions increases, lower temperatures cause particles to move slower
47
how does concentration affect the reaction rate
higher concentration means that there are more particles in the same amount of space, particles are more likely to collide and react
48
how does surface area affect the reaction rate
any reaction involving a solid can only take place on the surface of the solid, if surface area increases there are more collisions
49
how does a catalyst affect the reaction rate
it speeds up the reaction, the catalyst is unchanged/not used up by the end so isn't therefore a reactant and can be reused, it provides a surface for the reaction to take place on, therefore increases frequency of collisions
50
why are catalysts important in some industries
products are made more quickly, reduce the need for high temperatures, can be reused, essential for life, enzymes (biological catalysts)

dynamic science (2 decks)

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