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elements of life > structure of the atom > Flashcards

structure of the atom Flashcards

1
Q

what can a simple model of atomic structure explain

A

many chemical and nuclear processes

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2
Q

how many subatomic particles do atoms have

A

3

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3
Q

what are the three subatomic particles

A

proton
neutron
electron

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4
Q

what subatomic particles form the nucleus

A

protons and neutrons

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5
Q

what do the electrons do

A

orbit the nucleus in shells

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6
Q

what is the radius of most atoms

A

0.1nm

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7
Q

what is the radius of the nucleus

A

1x10^-15m

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8
Q

what is the mass of a proton

A

1

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9
Q

what is the mass of a neutron

A

1

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10
Q

what is the mass of an electron

A

0.00055

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11
Q

what is the charge of a proton

A

+1

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12
Q

what is the charge of a neutron

A

0

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13
Q

what is the charge of an electron

A

-1

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14
Q

what does the nucleus account for

A

most of the mass of an atom

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15
Q

why is an atom neutral overall

A

the number of protons = the number of electrons. the opposite and equal charges cancel each other out

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16
Q

which subatomic particle interacts in chemical reactions

A

electrons

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17
Q

how can we describe the nucleus

A

using the atomic number (Z) and mass number (A)

18
Q

what is the atomic number

A

the number of protons in the nucleus. it is numerically equal to the charge on the nucleus

19
Q

is the atomic number the same for every atom of an element

A

yes

20
Q

what is the mass number

A

the number of protons plus the number of neutrons in the nucleus

21
Q

what do nuclear symbols identify

A

the mass number and the atomic number as well as the symbol for the element

22
Q

what is the nuclear symbol for iodine

A

131
I
53

23
Q

what does the top number represent

A

the mass number

24
Q

what does the bottom number represent

A

atomic number

25
Q

why is the atomic number sometimes omitted in nuclear symbols

A

the chemical symbol tells us which element it is anyways

26
Q

what is an isotope

A

atoms of the same element with the same number of protons but different number of neutrons

27
Q

isotopes have the same atomic number but…

A

…different mass number

28
Q

what do most elements naturally exist of

A

isotopes

29
Q

what is the relative atomic mass of an element

A

an average of the masses taking into account their abundance

30
Q

how is it possible for chlorine to have 18.5 neutrons

A

atoms of the same element are not all identical, they can have a different mass.
the number of neutrons in the nucleus can vary - the mass number is therefore a weighted average

31
Q

do the number of protons and electrons change in isotopes

A

no

32
Q

how are isotopes written

A

by the symbol followed by the mass number

33
Q

the higher the number of neutrons…

A

…the greater the mass

34
Q

what does a higher number of neutrons tend to do

A

change physical properties slightly

35
Q

define relative isotopic mass

A

mass of isotope of atom compared with one twelfth of the mass of an atom of carbon-12

36
Q

define relative atomic mass

A

weighted mean mass of one atom of an element compared with one twelfth the mass of an atom of carbon-12

37
Q

how do you work out relative atomic mass

A

(mass x abundance) + (mass x abundance)
/ 100

38
Q

what is empirical formula

A

shows simplest whole number ratio of each type of atom

39
Q

steps to work out empirical formula

A
  • write each symbol
  • write each mass in g
  • write each Ar
  • find the number of moles
  • divide by the smallest number of moles
  • check for whole numbers
  • write the formula
40
Q

work out the empirical formula of an element containing 0.72g of Mg and 0.48g of O

A

Mg - 0.72/24 = 0.03 mol
O - 0.48/16 = 0.03

0.03/0.03 = 1
0.03/0.03 = 1
1:1 ratio
MgO

elements of life (15 decks)

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