Electron configuration Flashcards

1
Q

what is the formula for the main energy level

A

2n^2
where n is the number of the energy level so the first energy level holds two electrons the second holds 8

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2
Q

do the shapes of the electrons in the s d and p orbitals effect the shape of the molecule

why

A

yes

they represent a volume of space in which there is a 95% probability of finding an electron

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3
Q

what is the max amount of electrons any single atomic orbital can hold

A

2

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4
Q

how many groups do s-orbitals have

A

just one so there is still only 2 electrons

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5
Q

how many groups do p orbitals have

A

3 (still 2 electrons in each orbital) so in these 3 groups that will carry the same energy there will be 6 electrons in the p orbital

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6
Q

how many groups do the d orbitals have

A

5, each with the 2 electrons in the orbital of the same energy to give 10 in the d-sub level

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7
Q

note

A

in the orbital the electrons are a pair that are of the same negative charge so will try to move as far as possible from one another and this adds to the specific shape of the molecule

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8
Q

what is ionisation energy

A

the energy required to remove 1 mole of electrons from 1 mole of an atom in a gaseous state and is measured in KJmol-1

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9
Q

whta happens as a result of atoms being ionised

A

atoms become positive ions - cations

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10
Q

why is the first ionisation energy always the lowest

A

because it is being removed from a neutral atom - no electrons ahve been removed before

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11
Q

why is the second and so on ionisation energies higher than the first

A

because now you are removing electrons from a positive ion with charge it will now have a greater electrostatic force of attraction to the nucleus - it gains a successive ionisation energy as more electrons are removed because more energy will be required

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12
Q

what is the trend of ionisation energies on the periodic table

A
  • increases across a period because of an increase in nuclear charge from the protons and neutrons which will make it more difficult to remove an electron and requires more enrgy
  • increases up the group because the electrons are closer to the nucleus so the nuclear force of attraction is stronger
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13
Q

explain the decrease in first ionisation nergy between Mg- Al

A

the p orbital is higher in energy than the s orbital ( it is furtehr away from the nucleus

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