Chemistry For NursingClS 101

Course Content

• Introduction to Chemistry.• Water ( importance, features, and

structure).• Acids and Bases (most common,

features).• Liquid mixtures (types: solutions,

suspensions, colloids, and emulsions).

• Amino Acids: Classifications, features.

• Proteins: sources, functions, importance, level of structure, and classification.

Course Content

• Carbohydrates: Classification and origin.

Monosaccharide: common ones, structure, and chemical reactions.

Disaccharide: common ones, properties, and chemical reactions.

Polysaccharide: common ones and properties.

Course Contents• Lipids: Classifications, functions, and

importance.Fatty Acids: classifications and

properties.Simple lipids (fats, oils, and waxes):

chemical structures, features, importance, and chemical reactions.

Complex lipids (phosphoglycerides, sphingo lipids, and glycolipids): importance, and chemical structure.

Course Content

Derived lipids (prostaglandins and steroids).

Composition of cell membrane.

Refrences

Lippincott's Illustrated Reviews: BiochemistryPamela C. ChampeRichard A. Harvey

25% 1st Midterm25% 2nd Midterm

5% Quizzes5% Practical

40% Final exam

Introduction to Chemistry

AtomsAtom is the smallest portion of an element that can enter into chemical combination.

They cannot be bracken down or changed into another form by ordinary chemical and physical means. If placed side by side one million would stretch a distance of 1cm.

Atomic Theory

• John Dalton gave the atomic theory in 1808 which can be summarized

as: 1. All matter is made up of individual particles that are indivisible and

indestructible.

Atomic Theory

2. All atoms of a given element are

identical.3. Atoms of different

elements have different masses and

properties.

Atomic Theory

4. Atoms of elements combine in

simple ratios to form compounds.

5. A chemical reaction is a rearrangement of atoms.

Atomic Nucleus

• Atoms are normally electrically neutral.

• In 1909, Rutherford proposed that the atom consisted of tiny positively charged atomic nucleus with electrons outside

to produce electrically neutral atom.

Atomic Structure

At the center of the atom is a nucleus, which contains positively charged particles called protons, and noncharged particles called neutrons.In orbit outside the nucleus are electrons (negative charge)

Particle Charge Mass PROTON + Approximat

ely equal to that of

hydrogen atom.

NEUTRON NEUTRAL Approximately equal to

that of hydrogen

atomELECTRON - 1/1837 of a

hydrogen atom.

Energy Levels

The electrons of an tom orbit at specific distances from nucleus in regions called energy levels.The first level, the closest to the nucleus, can hold only two electrons.

The first level

The second energy level, the next in distance away from the nucleus, can hold 8 electrons.

More distant energy levels can hold 18 electrons.

Atomic structure

All of the protons and the neutrons

The 1st ring can hold up to 2 e-

The 2nd ring can hold up to 8 e-

The 3rd ring can hold up to 18 e-

The 4th ring and any after can hold up to 32 e-

• Draw a helium atom. Indicate where the protons, neutrons and electrons are.

+ +-

-

PROTONSNEUTRONS

ELECTRONS

ATOMIC # = 2 (PROTONS)

ATOMIC MASS = 4 (PROTONS & NEUTRONS)

Atomic Number

• Elements are different because they contain different numbers of PROTONS.

• The “atomic number” of an element is the number of protons in the nucleus.

• # protons in an atom = # of electrons.

Atomic Number

Element # of protons Atomic # (Z)

Carbon 6 6

Phosphorus 15 15

Gold 79 79

Simplest form of a substance -

cannot be broken down any further

without changing what it is.

There are 92 naturally occurring

elements.

20 additional elements have been

created in lab.

Elements

• Examples of elements hydrogen, mercury, gold

Isotopes

Isotopes are atoms of a given elements that differ in the number of neutrons.

OR

Isotopes are elements which have the same atomic number but different atomic weight.

For example, carbon-12, carbon-13 and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13 and 14 respectively.

The atomic number of carbon is 6 (every carbon atom has 6 protons); therefore the neutron numbers in these isotopes are 6, 7 and 8 respectively.

Mass Number

Mass number is the number of protons and neutrons in the nucleus of an isotope:Mass # = p+

+ n0

Nuclide p+ n0 e- Mass #

Oxygen - 10

- 33 42

- 31 15

8 8 1818

Arsenic 75 33 75

Phosphorus 15 3116

Complete Symbols

• Contain the symbol of the element, the mass number and the atomic number.

X Massnumber

Atomicnumber

Subscript →

Superscript →

The Periodic table

The periodic table is chart used by chemists to organize and describe the elements.

ClassificationGroups : A group is a vertical column in the periodic table. There are 18 groups.

Periods: A period is a horizontal row in the periodic table. There are 7 periods.

A molecule is formed when two or more atoms unite on the basis of their electron structures.

A molecule can be made of like atoms, but more often molecule is made of atoms of two or more different elements. Ex: water,

Molecules

Compounds

Chemical compound is a pure chemical

substance consisting of two or more different

chemical elements that can be separated into

simpler substances by chemical reactions.

What is the difference between a compound and a molecule?

A molecule is formed when two or more atoms join together chemically. A compound is a molecule that contains at least two different elements. All compounds are molecules but not all molecules are compounds.

Molecular hydrogen (H2), molecular oxygen (O2) and molecular nitrogen (N2) are not compounds because each is composed of a single element. Water (H2O), carbon dioxide (CO2) and methane (CH4) are compounds because each is made from more than one element.

TWO TYPES OF COMPOUNDS Organic molecules: Usually associated with living things. Always contain CARBON.Always have covalent bonds (share electrons)

Inorganic molecules:Any substance in which two or more chemical elements other than carbon are combined, nearly always in definite proportions• Water (H2O),

FORMULA

• The chemical symbols and numbers that compose a compound ("recipe")

• Structural Formula – Line drawings of the compound that shows the elements in proportion and how they are bonded

• Molecular Formula – the ACTUAL formula for a compound

C2H6O