Chemistry

Topic 1

Atomic Structure

Analytical Techniques

Isotopes

Flame Test, AES and AAS

Orbitals (electron config): 1s 2s 2p 3s 3p 4s 3d 4p ⭐

Every period is a new energy level

electrostatic attraction between protons and electrons

Electron configuration for isotope, removing or adding electrons to electron config

s (2 electrons) p (6 electrons) d (10 electrons)

Orbital diagrams, (boxes) arrows symbolize electrons ⭐

Rules for orbital diagrams

Aufbaus: Always fill the lowest one first

Hund: 1 arrow before 2

Paulis: Arrows (electrons) are in opposite ways

Atomic Notation image

Exceptions: Copper (Cu) and Chromium (Cr) ⭐

Why? Coppers electron config doesn't fill up its 3d orbital whereas Chromium doesn't fill the 3d orbital halfway, therefore creating creating it to be unstable

(X is also M)

Atoms and Isotopes

Ions

atomic number = p+ = e-

atomic mass - atomic number = n

atomic number = p+

atomic mass - atomic number = n

atomic number + or - ion charge = e-

Atoms: the smallest particle of a chemical element that can exist

Isotopes: same element/s with the same # of protons but different # of nuetrons (e.g. N7, N8, N9)

Ion: atom/molecule with electric charge due to their loss or gain of one or more electrons

In electron config, even though its 3p 4s 3d, electrons lose in orbital 4 and gains in orbital 3

Atoms that are heavy do not affect the size but the mass

if average atomic mass has a decimal place, the atoms are an isotopes??

Representation: e.g. Ni - 59 or Nickel - 59 ⭐

element or symbol name with the mass # :

different isotopes, same # of elements and protons but diff # of neutrons

physical property, same p and e = similar chemical properties

diff neutrons = diff physical properties (different mass = different density)

Relative atomic mass

It is the mass of the atom with respect to the mass of the isotope carbon - 12

Why carbon -12? atomic mass has a unit g/mol (gmol -1) but relative atomic mass does not

paired: 1s^2; unpaird 1s^1

Periodicity/Absorption

Mass Spectometry

Trends

Bonding

Atomic Radii

decreases across a period and increase down a group

Electronegativity

1st ionization energy

Ionic Radii

click to edit

Things on the data test

Formula writing and bonding is not on the test

Analytical Techniques

Identify Periodic Trends, patterns, relationships, limitations or uncertainty in data sets

No ionic formula writing or naming

do calculations of isotopic abundance/relative mass

isotopes -

remember acids (4)