Module 1 - Inorganic Chemistry

The study of matter, its properties, and the changes it may undergo

Chemistry

The study of inorganic substances used as medicines or in the preparation of pharmaceutical products

Inorganic pharmaceutical chemistry

Anything that occupies space and has mass

Matter

A form of matter that has a definite composition and distinct properties

Substance

T/F: The three states of matter can be interconverted without changing the composition of the substance

True

States of matter can be interconverted by what processes?

Heating, cooling

State of matter defined by rigidity and definite form/shape. Resists flow

Solid

State of matter having no definite shape and flow. It takes the shape of the container

Liquid

State of matter having no definite shape, can diffuse/spread/scatter to fill the container whenever placed. Particles tend to move independently of each other

Gas

It is the basic unit of a chemical element

Atom

A combination of two or more substances in which the substances retain their distinct identities

Mixture

A mixture wherein its composition is the same throughout (one phase - solution)

Homogenous mixture

A mixture wherein the composition is not uniform throughout (2 or more phases)

Heterogenous mixture

Metals/Non-metals: Loses electron/s and forms a cation

Metals

Metals/Non-metals: Gains electron/s and forms an anion

Non-metals

Categories of elements:

Lustrous and good conductors of heat and electricity

Metals

Categories of elements:

Non-lustrous, non-conductors of heat and electricity

Non-metals

Categories of elements:

Exhibits both properties of metals and non-metals

Metalloids

It is a substance that cannot be separated into simpler substances by chemical means

Element

The first theory of Dalton's Atomic Theory states

Elements are composed of extremely small particles called atoms

The second theory of Dalton's Atomic Theory states

Atoms of a given element are identical, having the same size, mass and chemical properties. The atoms of one element are different from the atoms of all other elements

The third theory of Dalton's Atomic Theory states

Compounds are composed of atoms of more than one element. The relative number of atoms of each element in a given compound is always the same

Law stating that different samples of the same compound always contain its constituent elements in the same proportion by mass

Law of definite proportions

Law of definite proportions is also called

Law of constant composition

Law of constant composition was published by

Joseph Proust

This law describes that if two elements can combine to form more than one compound, the masses of the one element that combine with a fixed mass of the other elements are in ratios of small whole numbers.

Law of multiple proportion

The fourth theory of Dalton's Atomic Theory states

Chemical reactions involve the rearrangement of atoms. Atoms are not created nor destroyed in a chemical reaction

Law that states that matter can neither be created nor destroyed during physical or chemical processes

Law of conservation of mass

This refers to the number of protons in the nucleus

Atomic number (Z)

The atomic number (Z) is found in the upper/lower left side of the chemical symbol

lower

This refers to the number of nucleons in a nucleus

Mass number

This refers to the number of protons + neutrons

Mass number/Atomic mass (A)

To get the number of neutrons:

Mass # - Atomic number

This refers to atoms of the same element with different number of neutrons in their nuclei

Isotopes

Atoms with the same atomic number but a different mass number

Isotopes

What are the three isotopes of H?

Protium, Deuterium, Tritium

Isotope of hydrogen also called "normal hydrogen", having a mass number of 1

Protium

Isotope of hydrogen also called "heavy hydrogen", having a mass number of 2

Deuterium

Isotope of hydrogen also referred to as the radioisotope, having a mass number of 3

Tritium

The two isotopes of uranium

235/92 U and 238/92 U

Isotope of uranium used for nuclear reactors and atomic bombs

235/92 U

This refers to nuclides with the same number of neutrons

Isotones

This refers to atoms with the same mass number

Isobars

This refers to either a proton or a neutron, considered in its roles as a component of an atomic nucleus

Nucleon

The number of nucleons is equal to the isotope's _______ aka nucleon number

mass number

How many neutrons are in 35/17 Cl?

18

How many neutrons are in 39/19 K?

20

Give the number of protons, electrons, and neutrons in 23/11 Na

11 protons, 11 electrons, 12 neutrons

Give the number of protons, electrons, and neutrons in 80/35 Br

35 protons, 35 electrons, 45 neutrons

It is a substance composed of atoms of two or more elements chemically united in fixed proportions

Compounds

General types of compounds:

Individual molecules composed of atoms (non-metals)

Molecular compound

General types of compounds:

Formed from ions that are either cation (+) or anion (-) (metal and non-metal)

Ionic compound

An aggregate of two or more atoms in a definite arrangement held together by chemical bonds

Molecule

A molecule that contains only two atoms of the same element or different elements

Diatomic molecule

A molecule that contains more than two atoms of the same element or different elements

Polyatomic molecule

Diatomic/Polyatomic: H₂

Diatomic

Diatomic/Polyatomic: H₂O

Polyatomic

Symbols and ratios of atoms for the elements in a chemical compound

Chemical formula

Chemical formula based on the actual molecule, gives the actual number of atoms of each element

Molecular formula

Chemical formula based on formula units, gives the smallest whole number ratio

Empirical formula, simplest formula

Chemical formula that shows the arrangement of atoms in a molecule of a compound, compounds are connected with dashes

Structural formula

Chemical formula based on the electron dot or lewis structure, a molecular structure in which the valency electrons are shown as dots so placed between bonded atoms that one pair of dots represents two electrons or one covalent (single) bond

Lewis formula

This refers to electrons available for bonding to achieve stability, also referred to as the electron/s found in the outermost shell of the atom

Valence electrons

This states that atoms lose or gain electrons to achieve a stable electronic configuration like the noble gases, except for helium

Octet Rule

He designed the periodic table of elements

Dmitri Mendeleev

Elements in the periodic table are arranged according to their increasing ____

atomic number

Elements in the periodic table are grouped based on their chemical properties/ _____

valence electrons

Group 1A outer configuration

s1

Group 2A outer configuration

s2

Group 3A outer configuration

s2p1

Group 4A outer configuration

s2p2

Group 5A outer configuration

s2p3

Group 6A outer configuration

s2p4

Group 7A outer configuration

s2p5

Group 8A outer configuration

s2p6

Group 1A # of valence electrons

1

Group 2A # of valence electrons

2

Group 3A # of valence electrons

3

Group 4A # of valence electrons

4

Group 5A # of valence electrons

5

Group 6A # of valence electrons

6

Group 7A # of valence electrons

7

Group 8A # of valence electrons

8

Group 1A Oxidation no./Valence

+1

Group 2A Oxidation no./Valence

+2

Group 3A Oxidation no./Valence

+3

Group 4A Oxidation no./Valence

+/-4

Group 5A Oxidation no./Valence

-3

Group 6A Oxidation no./Valence

-2

Group 7A Oxidation no./Valence

-1

Group 8A Oxidation no./Valence

0

Metal groups of elements

1A-3A

Metalloid group of elements

Grp 4A

Non-metal groups of elements

5A-7A

Stable group of elements

8A

Alkali Metal group

Group 1A

Alkali Earth Metal group

Group 2A

Boron group

Group 3A

Icosagen group

Group 3A

Carbon group

Group 4A