INORGANIC CHEMISTRY

matter

anything that takes up space and has mass

fixed volume and a fixed shape

solid in terms of volume and shape

has a fixed volume but variable shape

liquid in terms of volume and shape

has a variable shape and volume

gas in terms of volume and shape

as a pure substance or a mixture

matter can be divided based on complexity (2)

a molecule (if can be divided further), an atom (if cannot)

pure substance can be divided further into

heterogenous or homogenous form

mixture can further be divided into

compound or an element

a molecule can be further divided into

singular

atoms in terms of expressing the identity of a pure substance should be ______

singular or plural

elements n terms of expressing the identity of a pure substance can be ______

can be an element and an atom

Helium is what type of matter based on complexity

can be an molecule (plural) and element (2 atoms are of the same type)

Hydrogen gas is what type of matter based on complexity

can be a molecule and a compound

Sodium chloride is what type of matter based on complexity

neutral

uttering atom, element, molecule or compound often implies that a pure substance is what?

ion, which can either be based on the charge a cation or anion

if a substance have a charge what should it be preferably called

one (homogenous) or multiple (heterogenous) compositions

mixtures can be comprised of

solutions

most homogenous mixtures are

Law of Conservation of Mass (by Lavoiser)

Law of Definite Proportion/ Constant Composition (by Proust)

Law of Multiple Proportion (by Dalton)

in order to separate pure substances from mixtures, the three fundamental laws of chemistry were put to place

Law of conservation of mass (by Lavoiser)

the total mass of substance present after a chemical reaction is the same as the total mass before the reaction.

Law of Definite Proportion/ Constant composition (by Proust)

in a given substance, the relative numbers and kinds of atoms are constant in a ration of small whole numbers.

Law of Multiple Proportions (by Dalton)

when substances combine to from new produces (react) the mass of the elements are represented in the ratio of small shole numbers

molecular formula or empirical formula

when pure substances are written they are either written as

Molecular formula

written chemical formula that shows the exact number of atom

Empirical formula

written chemical formula that simplify atom counts to the lowest terms

Change

is a process that makes matter different from what it was, and is either visible or invisible.

Physical change

this property does not change the identity of matter

composition (e.g. whether things are mixed or separate)

tangible quantities like texture, viscosity, or color

actual physical states (solid, liquid ,gas)

properties that count for physical change include

melting

from solid to liquid the process is called

freezing

form liquid to solid the process is called

sublimation

from solid to gas the process is called

Deposition

from gas to solid the process is called

vaporization

from liquid to gas the process is called

condensation

from gas to liquid the process is called

Chemical change

this property does change the identity of the matter

atom

is the smallest identifiable unit of matter

neutron, proton, electron

what are the subatomic particles

Democritus

coined the term “atom” for the smalled identifiable unit of matter

John Dalton

formed the atomic theory (founded on the 3 fundamental laws of chemistry)

JJ Thomson

discovered the negatively charged electron via cathode-ray tube experiments, and assumed there are positively-charged particles balancing them out → plum pudding model

Ernest Rutherford (with Hans Geiger and Ernest Marsden)

confirmed the positively-charged protons through gold-foil experiments and proposed them to be concentrated in a small area (the nucleus) → nuclear model

James Chadwick

discovered the uncharged neutrons by bombarding beryllium with polonium

Robert Millikan

Measured the elementary electric charge (i.e. the real value of “-1” or “+1” in coulombs) through the oil drop experiment

Niels Bohr

Proposed that electrons reside in energy levels/ shells outside the nucleus → planetary model

Werner Heisenberg

Formulated the uncertainty principle, stating that one cannot accurately determine both the momentum and position of an electron at the same time (as if arguing the idea of fixed energy levels)

Erwin Schrodinger

Improved on Bohr’s ideas and devised the quantum model where electrons lie dynamically in electron clouds rather than fixed energy levels.

proton and neutrons

what are sometimes called “nucleons”

protons

atomic number is what subatomic particle

proton + neutron

mass number is what subatomic particle

atomic number is

position of the atomic number and atomic mass in the Elements

nuclide

the term for atoms when they have similar nucleons

Isotope

nuclide that has the same proton but different neutrons and mass number

Isotones

nuclide that has the same neutron but different proton and mass number

Isobars

nuclide that has the same atomic mass but different nucleons

orbital

is a space that accommodates 2 electrons

a node

is a section of the orbital that cannot hold electrons

subshell or sublevel

Multiple orbitals are grouped in a ________

whole energy level

multiple subshells constitutes a _______

(n)

symbol used to represent principal in Quantum Numbers

energy/shell

Principal (n) represents

1,2,3,4 and so on

Principal (n) numbers

(l)

symbol used to represent Azimuthal/ Angular in quantum numbers

shape of the orbital

sublevel/subshell

Azimuthal/ Angular (l) represents

s, 1, sphere

the name, number of orbitals, and the shape of the azimuthal 0

p, 3, dumbbell

the name, number of orbitals, and the shape of the azimuthal 1 have

d, 5, four leaf clover

the name, number of orbitals, and the shape of the azimuthal 2 have

f, 7, complex

the name, number of orbitals, and the shape of the azimuthal 3

m_l

the symbol used to represent magnetic in quantum numbers

the orientation of an orbital

Magnetic (m_l) represents

0 only

orientation of the orbital s

-1, 0, +1

orientation of the orbital p

-2, -1, 0, 1+, 2+

orientation of the orbital d

m_s

the symbol used to represent spin in quantum numbers

spin of an electron inside an orbital

spin (m_s) represent

+1/2 up arrow

-1/2 down arrow

spin (m_s) numbers

degenerate

starting from the p subshell, multiple orbitals of the same subshell have the same energies and are called as

Aufbau principle (madelung rule)

Hund’s rule (maximum multiplixity rule)

Pauli exclusion principle

principles concerned mainly with the principal and azimuthal numbers

Aufbau principle (Madelung rule)

in an atom with multiple energy levels and or sublevels, the electrons are filled up form 1s onward in a predictable fashion by order of increasing energy

Hund’s rule (Maximum multiplicity rule)

electrons fill up degenerate orbitals singly first (+1/2) before pairing up

Pauli exclusion principle

states that every electron in an atom is unique, no two electrons have the same set of quantum numbers

small

an atom electron configuration can be written at a complete form is the element is what

abbreviated form

an atom of a large element can be written at what form

valence

is the outermost (applies to shells subshells, or electrons)

Core

is the inner electrons (anything except the valence)

Octet rule

for smaller atoms, valence electrons of s and p block must be eight (octa) to be stable

Radioactivity

property to perform radioactive decay randomly

Radioactive decay

release of energy, which can be accompanied by change in the quantity of nucleons (either protons or neutrons)

alpha, beta, gamma

Three main types of radioactive decay

Alpha

decay in which the event it releases 2p and 2n losing 4

Beta

decay in which the event it releases 1e accompanied by conversion 1n to 1p resulting to no loss

gamma

decay in which the event it release high energy photons resulting into no loss

alpha

type of radioactive decay that have the least penetration (blocked by skin or paper)

alpha

type of radioactive decay that have the most ionization

Beta

type of radioactive decay that have a middle penetration (stopped by a sheet of aluminum)

Beta

type of radioactive decay that have a middle ionization

Gamma

type of radioactive decay that have the most penetration (stopped by thick layer of lead)

Gamma

type of radioactive decay that have the least ionization

Ci (curie)

common unit for radio activity

RAD (radiation absorbed dose)

common unit for absorbed dose

REM (roentgen equivalent man)

common unit for effective dose

R (roentgen)

common unit for exposure