Topic 1 Atomic Structure & Periodic Table Flashcards by Michael Slessor

What is the maximum number of electrons in each shell?

Shell 1 - 2
Shell 2 - 8
Shell 3 - 18
Shell 4 - 32
Shell 5 - 50

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How many sub shells are in each shell?

Shell 1 - 1
Shell 2 - 2
Shell 3 - 3
Shell 4 - 4

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What are the 4 different types of sub shells?

S, P, D and F orbitals

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What are the sub shells in each shell?

Shell 1 - 1s
Shell 2 - 2s, 2p
Shell 3 - 3s, 3p, 3d
Shell 4 - 4s, 4p, 4d, 4f

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What are the electron configurations of H, O, Na, Cl and Ca?

H - 1s(1)
O - 1s(2) 2s(2) 2p(4)
Na - 1s(2) 2s(2) 2p(6) 3s(1)
Cl - 1s(2) 2s(2) 2p(6) 3s(2) 3p(5)
Ca - 1s(2) 2s(2) 2p(6) 3s(2) 3p(6) 4s(2)

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What is the order of sub shells in the electron configuration?

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s …

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What is the Aufbau principle?

Electrons fill orbitals from the lowest energy first. This means the sub shells fill in this order: s, p, d, f.

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What is Hund’s rule?

Electrons will fill all orbitals with the same (up) spin first before filling the opposite (down) spin.

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How can you shorten electron configurations?

Put the noble gas before the element in square brackets then continue the electron configuration from there.

Cl:
Was - 1s(2) 2s(2) 2p(6) 3s(2) 3p(5)
Now - [Ne] 3s(2) 3p(5)

Ca:
Was - 1s(2) 2s(2) 2p(6) 3s(2) 3p(6) 4s(2)
Now - [Ar] 4s(2)

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How many orbitals are in each sub shell?

s - 1
p - 3
d - 5
f - 7

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What happens to the electron configuration when positive and negative ions are added?

Positive - Electrons are taken away from the highest energy level

Negative - Electrons are added to the highest energy level.

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When are electrons not removed/added to the highest energy level for an ion’s electron configuration?

When the element is in the transition metals. For example in elements in the first row of transition metals

Ti: [Ar] 4s(2) 3d(2)
Ti+: [Ar] 4s(1) 3d(2)
Ti2+: [Ar] 3d(2)

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What is the definition for relative atomic mass?

The average mass of 1 atom relative to 1/12th the mass of a 12C atom. (The Ar)

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What is the definition of relative isotopic mass?

The mass of an atom of the isotope relative to 1/12th the mass of a 12C atom.

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What is the definition of relative molecular mass?

The relative molecular mass of an element or compound is the sum of the relative atomic masses of all the atoms in its molecular formula. (The Mr)
E.g. O2 = 2 x (Ar of O) = 2 x 16 = 32

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What is the atomic number of an element?

The number of protons in the nucleus of an atom of the element.

What is an isotope of an element?

Atoms of an element with the same proton number (atomic number) but that differ with neutron number in the nucleus.

What is the mass number of an element?

The number of protons and neutrons in the nucleus of an atom of the element.

What are the relative masses of protons, neutrons and electrons?

Proton - 1
Neutron - 1
Electron - 1/1840

What are the relative charges of protons, neutrons and electrons?

Proton - +1
Neutron - 0
Electron - -1

What is the definition for relative formula mass?

The relative formula mass of a compound is the sum of the relative atomic masses of all the atoms in it’s formula. (The Mr)
E.g. Mg(NO3)2 = 24.3 + 2(14 + (16x3)) = 148.3

Why is relative formula mass used instead of relative molecular mass for metal compounds?

Relative formula mass is used because metal compounds consist of giant structures of ions and not molecules and this avoids the suggestion that their formulae are molecules.

What is an Orbital?

A region within an atom that can hold up to 2 electrons with opposite spins.

What are the shapes of S and P orbitals?

S - Sphere (Gets bigger for every shell e.g. 1s orbital is inside 2s orbital)

P - Dumbbell shaped (All 3 p orbitals are on each axis - x, y, and z.)

How do electrons fill orbitals?

Electrons fill orbitals singly (with up spins first) until all orbitals in the sub shell have one electron. At this point they fill the rest (with down spins).

How do you calculate relative atomic mass?

Total mass of all isotopes / Total number of isotopes e.g. Chlorine - Cl 35 and Cl 37 Relative Proportion: 3-1 (3 x 35) + (1 x 37) / 3 + 1 = 35.5

What does VIADD stand for?

Vaporisation, Ionisation, Acceleration, Deflection, Detection

When do you use VIADD?

To name the processes used in a mass spectrometer.

What is the definition of first ionisation energy?

The energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous positive ions.

What is the trend in first ionisation energy down a group?

The ionisation energy decreases because: - The filled inner shells provide a shielding affect which lowers the effective nuclear pull. - The size of the atom becomes greater, therefore the electron is further away from the nucleus which results in a lower nuclear attraction. As a result of this, less energy is needed to overcome the force of attraction from the nucleus.

What is the trend in first ionisation energy across a period?

The ionisation energy increases because: - The atom has a greater atomic number than the previous atom which results in a greater nuclear pull. As a result of this more energy is needed to overcome this force.

What is the definition for successive ionisation energy?

The energy required to remove one mole of electrons from one mole of gaseous unipositive ions to form one mole of gaseous dipositive ions.

How does the sub-shell that the electron is removed from affect the ionisation energy?

An electron in the highest energy level is more easily removed so has a lower ionisation energy. An electron in an intermediate energy level is harder to remove than that of one in the highest but easier than that of one in the lowest energy level so has intermediate ionisation energy. An electron in the lowest energy level is much harder to remove so has the highest ionisation energy.

What is shielding?

The effect of the inner electrons which reduces the pull of the nucleus on the electrons in the outer shell of an atom. Because of shielding, electrons in the outer shells are attracted by an 'effective nuclear charge' which is less than the full charge on the nucleus.

What are mass spectrometers used for?

They are used to determine the relative atomic mass of an element or compound.

How do mass spectrometers work?

Gaseous samples of elements or compounds are bombarded with high-energy electrons causing ionisation and resulting in positive ions being produced. The ions are accelerated by an electric field and bent into a circular path by a magnetic field. The radius of the path that different ions take depends on their mass. The ions are then detected and the number of ions at a particular mass can be determined.