Unit 2: The Chemical Level of Organization Part A: Basic Chemistry

Chemistry

Study of the composition, structure, and properties of matter

Matter

Anything that takes up space and has mass (weight)

Matter is made of

Elements

Element

Substance that cannot be broken down into other substances

Pure substance

Element

There are 92 naturally occurring

Elements

Chemical Symbol

The letter abbreviation for an element

C

Carbon

H

Hydrogen

K

Potassium

Ca

Calcium

O

Oxygen

N

Nitrogen

P

Phosphorus

S

Sulfur

Na

Sodium

Cl

Chlorin

Mg

Magnesium

Fe

Iron

Most abundant elements in the body

O, C, N, H, Ca, and P compose 98.5% of the body

Second most abundant are

K, S, Na, Cl, MG, Fe compose .8 of body

What elements compose .7% of the body

Trace elements

Atom

Smallest unit of matter

Nucleus

The center of an atom

Atom is made of ______ subatomic particles

Three

Protons

Have a positive charge and located within the nucleus of an atom

Neutrons

Have no charge and located within the nucleus of an atom

Electrons

Have a negative charge and located surrounding the nucleus in electron shells

An atom is electrically

Neutral

Atom is electrically neutral meaning

Number of electrons (negative charges) = number of protons (positive charges)

Atomic Number

The number of protons

Atomic Mass

The sum of protons and neutrons

Isotopes

Version of an element that has the same number of protons but a different number of neutrons, changing the mass.

Energy

The ability to do work

Work

The ability to move something Physiology Ex) bones such as when the body is moving, chemical bonds and atoms during a chemical reaction

2 forms of energy

Kinetic and Potential

Kinetic Energy

Energy of motion. It is energy that is doing work.

Kinetic Energy Examples

Anything with motion taking place (a moving car, water moving over waterfall, windmill turning, electricity as ions move)

Physiological examples of kinetic energy

Whole body movement, substances moving in and out of a cell

Potential energy

Energy of position, energy that is not doing work (at the moment) but has the potential to.

Think of Potential Energy as

Energy that is waiting to do work

Examples of potential energy

Water being held behind a dam, a stretched rubber band, a football quarterbacks arm before throwing the ball, energy in chemical bonds

Physiological example of potential energy

Ion and solutes being kept at a different concentrations on each side of the cell membrane and being prevented from moving across the cell membrane

Potential energy can be changed into

Kinetic energy and vise versa EX) quarterback throws ball and the potential energy is converted into kinetic energy

How many types of energy that are important in the body

Three

Chemical Energy (Important in body)

energy in chemical bonds.

Chemical Energy

Form is potential energy

Chemical Energy Example

Nutrient (food) molecules

Electrical energy

Energy from movement of ions

The form of electrical energy is

Kinetic energy

Electrical energy example

Electrical wires as they have copper ions in them, movements of ions in and out of a cell, batteries as they have several different ions like lithium

Electromagnetic energy

Energy of electromagnetic waves(invisible to eyes)

The form of electromagnetic energy is

Kinetic

Electromagnetic energy example

Light rays (includes visible light like UV light and infrared light) and X Rays

Matter is combined through

Chemical bonds and mixing

Chemical bond

A force holding atoms together

Molecule

Two or more atoms held together by a chemical bond

Chemical formula

An abbreviation for a molecule ex) O2 and S8

Compound

A special type of molecule that contains atoms of two or more different elements ex) h2o and c6h12o6

Isomer

Molecules with the same chemical formula but atoms are arranged differently. Ex) ethanol and ethyl ether, fructose and glucose and galactose.

Mixture

A substance made of two or more physically intermixed substances.

There are ___ types of mixtures

Four

Solution

A homogeneous and transparent mixture with small dissolved solute particles.

Solution Example

Sea water, Kool aid, Saline solution

Homogeneous

Evenly mixed

Transparent

Light can pass through and you can see through it

A solution has ___ parts

Two

Solvent

The substance that does the dissolving (always water for this course)

Solute

The dissolved substances, can be solids, gases, or other liquids.

Colloid

A heterogeneous and opaque mixture with large dissolved solute particles

Heterogeneous

Not evenly mixed

Opaque

Light cannot pass through and you cannot see through it

Colloid example

Jello, raw milk

Suspension

A heterogenous and opaque mixture with very large solute particles that aren’t completely dissolved so they sink to the bottom

Suspension example

Sand and water, blood, medications like amoxicillin.

Emulsion

A type of suspension where one liquid is suspended in another.

Emulsion example

Oil and vinegar, kaopectate or milk of magnesia

Can a substance be more than 1 type of solution

Yes. Ex) Blood is an NaCl solution, a colloid of proteins, and a suspension of cells.

There are ___ ways to measure solute concentration

Three

Weight per volume

The weight of solute per volume of solvent. Ex) 8.5g/l NaCl meaning 8.5 grams of NaCl per liter of water

Percentage

The percent solute relative to solvent. Ex) 5% of dextrose, meaning 5% dextrose and 95% water

Molarity

The number of molecules of solute per volume of solvent. Ex) expressed in units of M (molar) or mM (millimolar). 1M glucose

A chemical bond is a force holding atoms together, what is the force?

An energy relationship between electrons and different atoms

Valence Shell

The outer shell of an atom

The valence shell determines the ___ properties of an atom

Bonding

Chemically active elements

An atom with an unfulfilled valance shell actively looking to form bonds with other atoms to fill the valence shell.

Chemically Stable (inert) element

Will not form bonds because it’s valence shell is already filled

There are ___ types of chemical bonds?

Three

Ionic bond

Bond formed when atoms transfer electrons.

Cation

Atom loses electron(s) and becomes positively charge. It is the positively charged atom.

Anion

Negatively charged atom. This atom takes the anions lost electrons.

Cation and anion

This is an Ionic bond, as opposites attract. The loss/gain of electron and the force is the bond.

Ion

A charged atom. Ex) cation and anion, electrolytes, minerals

Ionic compound

A compound formed by an ionic bond. Ex) NaCl (table salt)

Covalent bond

A bond formed when atoms share pairs of electrons

Covalent bonds can be

Single, double, or triple bonds.

Single covalent bond

Atoms share one pair of electrons

Double covalent bonds

Atoms share two pairs of electrons

Triple covalent bonds

Atoms share three pairs of electrons

There are ___ types of covalent bonds

Two