Atomic structure

What is the definition for relative isotopic mass

the mass of an atom of a specific isotope which is relative to 1/12 of the mass of a carbon-12 atom

What is the definition of an isotope

an atom of an element that has the same number of protons but different number of neutrons

What the definition of relative atomic mass

the weighted mean of an atom of an element relative to 1/12 of the mass of a carbon -12 atom

What is ionisation energy?

The amount of energy needed to remove 1 mol of electrons from 1 mol of a gas.

What is formed when 1 mol of electrons is removed from a gas?

1+ ions.

Relative mass of an electron

1/1836

What is First ionisation energy

The energy required to remove 1 mol of electrons from each atom in 1 mole of gaseous atoms to form 1 mol of gaseous 1+ I

Name one factor that affects ionisation energy

no. of protons i.e. charge of the nucleus

Name another factor that affects ionisation energies

Atomic radius

Name the last factor that affects ionisation energy

Electron shielding

What group of elements are always in the trough of first ionisation energies

group 1

Which element are always at the peak of first ionisation energies

group 0/8

What's the general trend for first ionisation energies across a period

increase

How does the first ionisation energy change down a group

decreases

why do isotopes have the same chemical properties

Because they have the same electron configuration

Why do isotopes have the same physical properties

They have different masses

What happens to the ionisation energy as you keep removing electrons

it increases

What block is group 1 and 2 of the periodic table

The S block

What block is transition metals?

The D block

What block are groups 3-8

The P block

What shape is an s orbital

Spherical

What shape is a p orbital

Dumbell shaped

Definition of an orbital

A region in space where there is a 95% chance to find an electron. Each orbital can hold up to two electrons with opposite spins

What are the man stages of mass spectrometry

1. Ionisation - sample atoms bombarded by high energy electrons 2. Acceleration - ions accelerated by an electric field. 3. Deflection - ions are deflected by a magnetic field based on mass:charge 4. Detection - ions hit a detector and produce a signal proportional to abundance.

How are ions accelerated in mass spectrometry

All the ions are accelerated by and electric field so they all have the same kinetic energy. Lighter ions moved faster and heavy ions slower

How are ions deflected in mass spectrometry

Based off mass:charge. A light ion is deflected more. A heavy ion is deflected less. An ion with lots of charge is deflected more