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chemistry 2 > atomic structure p1 > Flashcards

atomic structure p1 Flashcards

1
Q

explain the current model of the atom

A
  • protons and neutrons are found in the nucleus
  • electrons orbit the nucleus in shells
  • the nucleus is tiny compared to the total volume of atom
  • most of atom’s mass is in the nucleus
  • most of the atom is empty space between the nucleus and the electrons
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2
Q

what is the charge of a proton and an electron?

A

proton = +1
electron = -1

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3
Q

which particle has the same mass as proton?

A

neutron

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4
Q

which two particles make up most of atom’s mass?

A

protons and neutrons

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5
Q

what does the atomic number show about an element?

A

atomic number = number of protons in an atom

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6
Q

how is the mass number calculated?

A

mass number = number of protons + number of neutrons

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7
Q

isotope

A

atoms of the same element with different number of neutrons and therefore different mass number

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8
Q

why do different isotopes of the same element react in the same way?

A
  • neutrons have no impact on the chemical reactivity
  • reactions involve electrons, isotopes have the same number of electrons in the same arrangement
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9
Q

relative atomic mass

A

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

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10
Q

relative isotopic mass

A

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

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11
Q

the relative isotopic mass is same as which number?

A

mass number

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12
Q

what two assumptions are made when calculating mass number?

A
  • contribution of the electron is neglected
  • mass of both proton and neutron is taken as 1.0
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13
Q

how to calculate the relative molecular mass and relative formula mass?

A

both can be calculated by adding the relative atomic masses of each of the atom making up the molecule or the formula

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14
Q

what are the uses of mass spectrometry?

A
  • identify unknown compounds
  • find relative abundance of each isotope of an element
  • determine structural information
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15
Q

what is the m/z value of the M+ ion from a graph??

A

last peak

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16
Q

what does the principal quantum number indicate?

A

the shell occupied by the electrons

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17
Q

what is a shell?

A

a group of orbitals with the same principal quantum number

18
Q

how many electrons can each shell hold?

A

1st - 2
2nd - 8
3rd - 18
4th - 32

19
Q

what is an orbital?

A

a region around the nucleus that can hold up to two electrons with opposite spin
95% (?) chance of finding an electron

20
Q

what are the four types of orbitals?

A

s, p, d, f

21
Q

what shape are the orbitals?

A

s - spherical
p - dumb bell

22
Q

how many orbitals are present in each sub shell?

A

s - 1, 2 electrons
p - 3, 6 electrons
d - 5, 10 electrons
f - 7, 14 electrons

23
Q

what rules are electrons arranged in a shell by?

A
  • electrons are added one at a time
  • lowest available energy level is filled first
  • each energy level must be filled before the next one can fill
  • each orbital is filled singly before pairing
  • 4s is filled before 3d
24
Q

why does 4s orbital fill before 3d orbital?

A

4s has a lower energy than 3d before it is filled

25
Q

how can the electron configuration be written in short?

A

the noble gas before the element used to abbreviate
(often [Ar])

26
Q

how are the elements arranged in a periodic table?

A

they are arranged in the order of increasing atomic numbers

27
Q

what is a period on a periodic table?

A

horizontal rows

28
Q

what is a group on a periodic table?

A

vertical columns

29
Q

how is the group number related to the number of electrons?

A

group number = number of electrons in outer shell

30
Q

what is meant by periodicity?

A

the repeating trends in chemical and physical properties

31
Q

first ionisation energy

A

the energy required to remove a mole of electrons from a mole of gaseous atoms to form one mole of gaseous 1+ ion under standard conditions

32
Q

first ionisation energy equation of Mg

A

Mg(g) –> Mg+(g) + e-

33
Q

what are the factors that affect ionisation energy?

A
  • atomic radius
  • nuclear charge
  • electron shielding or screening
34
Q

why does ionisation energy increase across a period?

A

increased nuclear charge, decreased atomic radius, same electron shielding
more energy needed to remove first electron

35
Q

why does first ionisation energy decrease between group 2 to 3?

A

decreases between 2 to 3 because in group 3 the outermost electrons are in p orbitals
whereas in group 2 they are in the s orbital so the electrons are easier to remove from p as it is further from the nucleus

36
Q

why does first ionisation energy decrease between groups 5 and 6?

A

decrease due to the group 5 electrons in p orbital which are single electrons
in group 6 the outermost electrons are spin paired, with some repulsion
therefore the electrons are slightly easier to remove

37
Q

does first ionisation increase or decrease between the end of one period and the start of the next? why?

A

decrease
there is increase in atomic radius
increase in electron shielding

38
Q

does first ionisation increase or decrease down a group? why?

A

decrease
shielding increases, atomic radius increases, nuclear charge increases however outweighed by radius and shielding

39
Q

describe the structure, forces and bonding in every element across period 2? (Li, Be, B, C, N, O, F, Ne)

A

Li & Be –> giant metallic; strong attraction between positive ions and delocalised electrons; metallic bonding
B & C –> giant covalent; strong forces between atoms; covalent
N2, O2, F2, Ne –> simple molecular; weak intermolecular forces between molecules; covalent bonding within molecules and intermolecular forces between molecules

40
Q

describe the structure, forces and bonding in every element across period 3: Na, Mg, Al, Si, P, S, Cl, Ar

A

Na, Mg, Al –> giant metallic; strong attraction between positive ions and delocalised electrons; metallic bonding
Si –> giant covalent; strong forces between atoms; covalent
P4, S8, Cl2, Ar –> simple molecular; weak intermolecular forces between molecules and intermolecular forces between molecules

41
Q

what are the 4 stages of mass spec?

A

1 - ionisation - element is vaporised and injected into the mass spec where a high voltage is passed over the chamber causing electrons to be removed leaving +1 charged ions
2 - acceleration
3 - ion drift - ions deflected by a magnetic field into a curved path
4 - detection - positive ions hit negatively charged detection plate, gaining an electron and producing a flow of charge - the greater the abundance the greater the current produced

5 - analysis

chemistry 2 (21 decks)

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