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atomic structure Flashcards

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1
Q

define an atom.

A

the smallest particle of a chemical element that can exist.

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2
Q

define an element.

A

a pure substance made of only one kind of atom

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3
Q

what is a compound?

A

a substance made up of atoms of two or more different elements joined by chemical bonds

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4
Q

what is the difference between a mixture and compound?

A

a mixture combination of two or more different substances that are NOT joined by chemical bonds

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5
Q

what is a molecule?

A

a group of atoms bonded together (can be the same type of atom, or different types of atom)- eg CO2, H2O

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5
Q

what is the relative mass of a proton?

A

1

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6
Q

what is the relative mass of a neutron?

A

1

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7
Q

what is the relative mass of an electron?

A

roughly 1/1836- negligible

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8
Q

what is the relative charge of a proton?

A

+1

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9
Q

what is the relative charge of a neutron?

A

0

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10
Q

what is the relative charge of an electron?

A

-1

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11
Q

what is the atomic number?

A

the number of protons in the nucleus of an atom

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12
Q

where are each of the subatomic particles found?

A

protons and neutrons in the nucleus, electrons in shells orbiting the nucleus

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13
Q

what is the average radius of an atom?

A

0.1 nm (1 x 10^-10 m)

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14
Q

what is the average radius of the nucleus

A

10000 times smaller than atom- 1 x 10^-14 m

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15
Q

how do you find the number of neutrons in an atom?

A

mass number - atomic number

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16
Q

define isotope

A

atoms of the same element that have different numbers of neutrons

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17
Q

what does the number of electron shells correspond to?

A

the period (horizontal row) on the periodic table

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18
Q

what is a valence electron?

A

electrons on the outer shell that are involved in reactions

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19
Q

what do outer shell electrons correspond to?

A

group number in periodic table

20
Q

what was john dalton’s theory of atoms?

A

believed that atoms could not be divided, but were rearranged in chemical reactions

21
Q

what did john newland find?

A

noticed a repeating pattern every 8 elements and suggested elements were found in ‘octaves’

22
Q

what were elements ordered by historically?

A

atomic weight

23
Q

what are elements ordered by now?

A

atomic number (number of protons)

24
Q

what were dmitri mendeleev’s ideas?

A

he ordered elements by atomic weight BUT changed the order/left gaps to keep elements with similar properties in the same column

25
Q

what were the advantages of mendeleev’s ideas?

A

was able to predict properties of elements in the gaps, eg germanium

26
Q

what charge ions do metals form?

A

positive

27
Q

what charge do non-metals form?

A

negative

28
Q

what are some properties of metals?

A

shiny, malleable, ductile, good conductors of heat and electricity

29
Q

what are some properties of non-metals?

A

dull, brittle, insulators of heat and electricity, liquids and gases at room temperature

30
Q

what is the pH of metal oxides?

A

acidic

31
Q

what is the pH of non-metal oxides?

A

alkaline

32
Q

what are in group 0?

A

noble gases- helium, argon, neon

33
Q

describe the electron structure of group 0 elements

A

all have full shells of electrons- stable and very unreactive (inert)

34
Q

what are group 0 physical properties?

A

all colorless gases at room temperature

35
Q

what is the pattern for boiling point of group 0?

A

boiling point increases going down the group- larger atoms, more IMF, more energy required to overcome

36
Q

what elements are in group 1?

A

alkali metals- sodium. lithium, potassium

37
Q

what is the pattern for reactivity in group 1?

A

increases going down the group- one outer shell electron is further from the nucleus so it is less attracted (receives less shielding) so it is easier to lose.

38
Q

metal + water -> ???

A

metal hydroxide + oxygen

39
Q

what are the group 7 elements known as?

A

halogens

40
Q

what are diatomic molecules?

A

molecules of atoms that travel in pairs- hydrogen (H), nitrogen (N), oxygen (O), fluorine (F), chlorine (Cl), bromine (Br), and iodine (I)

41
Q

what is the pattern in boiling and melting points for halogens?

A

increase going down the group- more IMF

42
Q

what is the reactivity pattern for halogens?

A

get less reactive- larger atomic radius, more shielding, less nuclear attraction, harder to gain an electron

43
Q

why will sodium chloride + bromine not react?

A

displacement reaction will NOT occur since chlorine is more reactive than bromine

44
Q

describe chemical and physical properties of transition metals

A

slow/no reaction with o2, water and halogens
hard, high melting points, strong+ dense

45
Q

describe charges on transition metal ions

A

form positive ions often with the ability to form more than one ion

46
Q

why are transition metals good catalysts?

A

because they can form more than one ion

47
Q

what makes transition metals special?

A

they have an incomplete sub-shell as well as an incomplete outer shell, giving them specialised properties eg colors

chemistry (10 decks)

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