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Flashcards in Atomic Structure Deck (18)
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1
Q

What is an orbital?

A

A region that can hold up to two electrons with opposite spins

2
Q

What is the shape of an s-orbital?

A

Spherical

3
Q

What is the Shape of a p-orbital?

A

Dumbell

4
Q

What is the first ionisation energy?

A

Is the enthalpy change when ONE MOLE of electrons is removed from ONE MOLE of gaseous atoms to form ONE MOLE of gaseous positive ions

5
Q

What is the successive ionisation energy?

A

Successive ionisation energies are a measure of the energy required to remove each electron in turn from an atom

6
Q

What is Aufbau Principle?

A

Electrons will fill lower energy orbitals before higher energy ones

7
Q

What is the Pauli Exclusion Principle?

A

No to electrons can have the same four quantum numbers. The means that electrons in the same orbital have opposite spins

8
Q

What is Hund’s rule?

A

Every orbital in a sub shell (s,p,d,f) is singly occupied before any orbital is doubly occupied. Electrons in singly occupied orbitals will have the same spin.

9
Q

What is the difference between shells, sub shells and orbitals?

A
  • Shells are the principle quantum number/ energy level (1,2,3 or 4)
  • A sub shell is what each shell is split into: s,p,d,f and with each shell you gain a sub shell
  • Orbitals are regions that can hold up to tow electrons with opposite spins so:
    1. The s subshell has 1 orbital and so can hold 2 electrons
    2. The p sub shell has 3 orbitals and so can hold 6 electrons
    3. The d sub shell has 5 orbitals and so can hold 10 electrons
    4. The f sub shell has 7 orbitals and so can hold 14 electrons
  • Only 2 electrons max. can be in a orbital!
10
Q

What factors affect ionisation energy?

A
  1. Distance from the nucleus
  2. Nuclear Charge
  3. Shielding
  4. Charge on ion
11
Q

What is an isotope?

A

Isotopes are atoms of the same element with different numbers of neutrons and therefore different mass numbers. The atomic number remains the same

12
Q

What is the relative isotopic mass?

A

The mass of an isotope relative to 1/12th of the mass of an atom of carbon-12

13
Q

What is the relative atomic mass?

A

The man mass of an element relative to 1/12th the mass of an atom of carbon-12

14
Q

What is the relative molecular mass?

A

The sum of the relative atomic masses in simple covalent molecules and diatomic elements e.g. nitrogen (N2)

15
Q

What is the relative formula mass?

A

The sum of the relative atomic masses in compounds with giant structures e.g. sodium chloride

16
Q

Why are the second ionisation energies of calcium and strontium greater than their first ionisation energies?

A

Removing an electron from a more positive ion

17
Q

Why do successive ionisation energies increase with ionisation number?

A
  1. Radius decreases

2. Attraction between (the remaining) electron and nucleus increases

18
Q

How do the first ionisation energies of Mg (738) and Al (578) show details of electron structure?

A
  1. Mg has oute electron in 3s sub shell
  2. Al has outer electron in 3p sub shell
  3. 3p subshell has higher energy than 3s sub shell