Atomic structure, spectra and electron configurations Flashcards

EL1

1
Q

what are atoms made from?

A

protons, neutrons and electrons

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2
Q

give the characteristics of an electron

A
  • electrons have a -1 charge
  • they wizz around the nucleus in shells, these shells take up most of the volume of the atom
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3
Q

give the characteristics of the nucleus

A
  • most of the mass of the atom is concentrated in the nucleus
  • the diameter of the nucleus is rather titchy when compared to the whole atom
  • the nucleus is where you find the protons and neutrons
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4
Q

whats the relative charge and mass of a proton?

A

charge: +1
mass: 1

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5
Q

whats the relative charge and mass of a neutron?

A

charge: 0
mass: 1

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6
Q

whats the relative charge and mass of an electron?

A

charges: -1
mass: 1/2000 (negligible)

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7
Q

what do ions have different numbers of?

A

ions have different numbers of protons and electrons
- negative ions have more electrons than protons
- positive ions have fewer electrons than protons

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8
Q

what are isotopes?

A

isotopes are atoms of the same element with different numbers of neutrons

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9
Q

describe the nuclear model and how Rutherford proved this?

A
  • a tiny, positively charged nucleus at the centre, surrounded by a cloud of negative electrons. most of the atom is empty space
  • Rutherford fired alpha particles at a thin sheet of gold, the expectation was that most would be very slightly deflected but in fact almost all passed directly through and a very small number were deflected. this proved the plum pudding model incorrect and made the nuclear model.
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10
Q

describe the plum pudding model

A

a positively charged sphere with negative electrons embedded in it

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11
Q

describe the bohr model

A
  • electrons exist in fixed orbits, or shells and not anywhere in between.
  • each shell has a fixed energy
  • when an electron moves between shells electromagnetic radiation is emitted or absorbed
  • because the energy of the shells is fixed, the radiation will have a fixed frequency
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12
Q

what particle did J J Thompson discover?

A

the electron

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13
Q

what is relative atomic mass?

A

relative atomic mass is the mean weighted mass of an atom of an element compared with the 1/12th the mass of an atom of carbon-12

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14
Q

what is relative molecular mass?

A

relative molecular mass is the mean weighted mass of a molecule compared with 1/12th the mass of an atom of carbon-12

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15
Q

what is relative formula mass?

A

relative atomic mass is the sum of the mean weighted masses of all atoms in the formula of a compound compared with 1/12th the mass of an atom of carbon-12

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16
Q

what is a mole?

A

a mole is the amount of substance containing as many particles as there are atoms in 12g of carbon-12

17
Q

what is an ionic equation?

A

an ionic equation is an equation in which only the non-spectating ions are shown

18
Q

how is percentage yield calculated?

A

= (actual yield/expected yield) x 100

19
Q

how is percentage composition by mass calculated?

A

= (mass of desired substance/mass of mixture) x 100

20
Q

how is a standard solution prepared from a concentrated solution?

A
  • a certain volume of the concentrated solution is added to a volumetric flask in order to get the desired final volume
  • distilled water is added to the volumetric flask up to the line on its neck
21
Q

how do you calculate the mass spectrometry of an element?

A

(%abundance x mass number) + same for all other isotopes / 100

22
Q

describe empirical and molecular formulas?

A

empirical: the simplest ratio of all the elements present in the simplest formula
molecular: the actual number of each type of atom present in one molecule of a compound

23
Q

define atom?

A

smallest piece of an element, contains protons and neutrons and is overall neutral

24
Q

what is a group and a period on the periodic table?

A

Group: a vertical column in the periodic table, same number of electrons in outer shell
Period: a horizontal row of elements in the periodic table, all with the same number of electron shells

25
Q
A