H2 Chem Chp 3 Atomic Structure

what is the angle of deflection?

k|charge/mass|

what are the types of s orbitals?

s

what are the types of p orbitals?

px, py, pz

what are the types of d orbitals?

dxy, dyz, dxz, dx2-y2, dz2

draw all the d orbitals. which one has a unique shape?

dz2: has a dumbbell shape with collar

what is the rule for arrangement of atoms?

1. Aufbau principle

2. Pauli’s Exclusion Principle

3. Hund’s Rule

whats aufbau principle?

Electrons occupy the lowest energy orbital first before occupying higher energy orbitals

whats pauli’s exclusion principle?

each orbital can hold a maximum of 2 electrons. the 2 electrons must be in opposite spins

what’s hund’s rule?

degenerate orbitals must be occupied singly by electrons with parallel spins before pairing occurs to minimise electron repulsion

what are the exceptions to writing electronic configurations?

Cr and Cu

what is the electronic config of Cr? and why?

1s2 2s2 2p6 3s2 3p6 3d5 4s1. Cr gains extra stability with a half filled 3d subshell

what is the electronic config of Cu? and why?

1s2 2s2 2p6 3s2 3p6 3d10 4s1. Cu gains extra stability with a fully filled 3d subshell.

what is the first ionisation energy?

Energy required to remove 1 mole of electrons from 1 mole of gaseous atoms of the element to form 1 mole of singly positively charged gaseous ions

whats first IE eqn for element X. ALWAYS write state symbols!

x(g）→ x+(g) + e-

what is the second ionisation energy?

Energy required to remove 1 mole of electrons from 1 mole of singly positively charged gaseous ions to form 1 mole of doubly positively charged gaseous ions

whats 2nd IE eqn for element X. ALWAYS write state symbols!

X+(g) → X2+(g)+ e-

what does Mg(g)→ Mg2+(g) + 2e- represent?

the sum of the first and second ionisation energies

why is the 2nd IE higher than the first IE?

more energy is required to remove an electron from a positively charged ion compared to a neutral atom due to stronger net electrostatic attraction

• stronger effective nuclear charge of electrons of positively charged ion

what are the factors affecting ionisation energies of elements?

• nuclear charge

• screening effect

what is nuclear charge

the attractive force of protons in the nucleus for electrons

whats