Thanato Midterm

Chemistry

The science of substances, their structure, composition, and reactions.

Organic Chemistry

Study of carbon compounds.

Inorganic Chemistry

Study of non-carbon elements.

Biochemistry

the study of chemical processes in living organisms.

Analytical Chemistry

Qualitative (what is it?) and quantitative (how much?) analysis.

Physical Chemistry

Physical nature of matter, bonds, and structures.

Radiochemistry

Chemistry of radioactive matter.

Embalming Chemistry

Chemical processes in dead organic matter for preservation.

Matter

Anything with mass, inertia, and that occupies space.

Inertia

Resistance to change in motion (Newton's First Law).

Force

Cause of motion or change in motion.

Acceleration

Rate of change in velocity.

Mass

Measure of inertia.

Weight

Mass under gravity.

Meter

Base unit of length in metric/SI system.

Liter

Unit of volume (derived from meter).

Kilogram

Base unit of mass.

Density

Mass per unit volume.

Specific Gravity

Density of object relative to water.

Temperature

Measure of heat intensity; scales: Fahrenheit (°F), Celsius (°C), Kelvin (K).

Heat

Energy causing temperature change; measured in calories.

Calorie

Heat to raise 1g water by 1°C.

Kilocalorie

1000 calories.

Energy

Capacity to do work; types: kinetic (motion), potential (stored).

Exothermic

Process releasing heat.

Endothermic

Process absorbing heat.

Law of Conservation of Energy

Energy is neither created nor destroyed.

Law of Conservation of Mass

Mass is neither created nor destroyed.

Law of Conservation of Mass and Energy

Mass and energy can interconvert (E = mc²).

Chemical Property

Characteristic observed by changing the substance's identity (e.g., flammability).

Physical Property

Characteristic observed without changing identity (e.g., color, odor, density).

States of Matter

Solid (definite shape/volume), liquid (definite volume, no shape), gas (no definite shape/volume).

Sublimation

Solid to gas without liquid phase (e.g., dry ice).

Physical Change

Alters form, not composition (e.g., freezing).

Chemical Change

Alters composition, forms new substances (e.g., burning).

Element

Pure substance, cannot be decomposed chemically; unique properties.

Compound

Two+ elements chemically combined in fixed proportions.

Mixture

Physical combination; homogeneous (uniform, e.g., solutions) or heterogeneous (non-uniform).

Metal

Luster, ductile, malleable, good conductor, solid (mostly), positive charge.

Non-metal elements

No luster, brittle, poor conductor, various states, negative charge.

Atomic Symbol

Abbreviation for element (e.g., Fe for iron).

Isotope

Atoms of same element with different neutrons (e.g., H isotopes: protium, deuterium, tritium).

Atomic Weight

Sum of protons, neutrons, electrons (approx. mass number = protons + neutrons).

Subatomic Particles

Proton (+1, nucleus), neutron (0, nucleus), electron (-1, orbits).

Electronic Configuration

Arrangement of electrons in shells/orbits (e.g., 1s² 2s² 2p⁶…).

Shell

Energy level (K, L, M…); max electrons = 2n².

Orbit

Sub-level (s, p, d, f).

Valence Electrons

Outermost shell electrons; determine properties.

Periodic Table

Arranged by atomic number; periods (rows = outer shell), groups (columns = valence electrons)

Specific gravity of blood

1.041 - 1.067 (unitless)

Why study chemistry?

Explains the composition & changes of matter. Foundation for biology, medicine, embalming, etc. Practical applications in daily life (health, environment, industry)

Families in the Periodic Table

Group I (alkalis), Group VII (halogens), Group VIII/0 (noble gases)

Neutrons

Atomic Mass - Atomic Number

Max electrons in shell

2n² (n = shell number)

Protons

Atomic Number

Protons

Atomic Number

Chemical Bonding

Method holding compounds together

Ionic Bond

Transfer of electrons, attraction of opposite charges (electrovalent)

Covalent Bond

Sharing of electrons

Electronegativity

Attraction for valence electrons

Ion

Charged atom; cation (+, loses e-), anion (-, gains e-)

Monatomic Ion

Single atom ion

Polyatomic Ion (Radical)

Multi-atom ion (e.g., NH4^+)

Single Bond

1 pair shared (2 e-)

Double Bond

2 pairs shared (4 e-)

Triple Bond

3 pairs shared (6 e-)

Polar Bond

Unequal sharing, partial charges (e.g., H2O)

Dipole

Two polar bonds forming partial charges

Oxidation Number (Valence)

Electrons lost/gained/shared; combining capacity

Common Polyatomic Ions

Ammonium NH4 +1, Hydroxide OH -1, Nitrate NO3 -1, Sulfate SO4 -2, Phosphate PO4 -3

Metal Elements

Luster, ductile, malleable, good conductors, solid (mostly), positive charge

Non-Metal Elements

No luster, brittle, poor conductors, various states, negative charge

Noble Gases

No charge, gaseous, inert (e.g., He, Ne, Kr, Rn)

Hydrogen

Water-former, diatomic (H2), nascent (single H), positive charge, reducing agent

Molecular Hydrogen

H2, colorless/odorless

Nascent Hydrogen

Single H atom

Oxygen

Acid former, diatomic (O2), nascent (O), ozone (O3), oxidizing agent

Reduction

Removal of O, addition of H, gain of e-, decrease in valence

Oxidation

Addition of O, removal of H, loss of e-, increase in valence

Slow Oxidation

Low temp (e.g., rusting)

Rapid Oxidation (Combustion)

High temp (e.g., burning)

Spontaneous Combustion

Unvented heat buildup

Decay

Slow oxidation by aerobic bacteria

Putrefaction

Slow oxidation by anaerobic bacteria

Kindling Point

Temp at which substance bursts into flame

Luster (Metal)

Shiny surface

Ductility (Metal)

Formed into wires

Malleability (Metal)

Formed into sheets

Conductivity (Metal)

Good for heat/electricity

State (Metal)

Solid at room temp

Saprophytic bacteria

Normally resides in the digestive tract and uses dead organic matter as nutritional sources after death.

Enzyme inhibition

Two ways enzymes can be inhibited by certain molecules: Competitive and noncompetitive.

Ammonia

The product of putrefaction, which has an impact on the embalming process.

Organic enzyme

A compound that normally acts as a catalyst for some type of chemical reaction such as hydrolysis.

Denaturation

The disruption and breakdown of a protein by heat or chemicals.

Arrhenius theory

States that acids break apart in a water solution to yield hydrogen ions.

Lewis Theory

An acid is any substance that accepts a pair of electrons and a base is any substance that donates a pair of electrons.

Types of formulas

General, structural, molecular, and line.

Benzene

A ring of six carbons with alternating double bonds between the carbons and a single hydrogen attached to each carbon.

Radical

A molecule that contains at least one unpaired electron.