Anatomy And Physiology (Chapter 2)

Front 1

Matter

Back 1

Anything that occupies space and has mass (weight).

Front 2

Elements

Back 2

Fundamental units of matter.

*96% of the body is made from four elements:

- Carbon (C)

- Oxygen (O)

- Hydrogen (H)

- Nitrogen (N)

Front 3

Atoms

Back 3

Building blocks of elements; unique substances that cannot be broken down into simpler substances by ordinary chemical methods.

Front 4

Nucleus

Back 4

A dense body in most cells containing the genetic material of the cell.

Front 5

Proton

Back 5

Subatomic particle that bears a positive charge; located in the atomic nucleus.

Front 6

Neutron

Back 6

Uncharged subatomic particle.

Front 7

Electron

Back 7

Negatively charged subatomic particle.

Front 8

Atomic Number

Back 8

Equal to the number of protons that the atom contains.

Front 9

Atomic Mass Number

Back 9

Sum of the protons and neutrons.

Front 10

Atomic Weight

Back 10

Close to mass number of most abundant isotope; reflects natural isotope variation.

Front 11

Isotopes

Back 11

Different atomic form of the same element - vary only in the number of neutrons they contain.

Front 12

Radioisotope

Back 12

- heavy isotope

- tends to be unstable

- decomposes to more stable isotope

Front 13

Radioactivity

Back 13

Process of spontaneous atomic decay.

Front 14

Molecule

Back 14

Two or more like atoms combined chemically.

Front 15

Compound

Back 15

Two or more different atoms combined chemically.

Front 16

Chemical Reactions

Back 16

- Atoms are united by chemical bonds

- Atoms dissociate from other atoms when chemical bonds are broken

Front 17

Electrons

Back 17

- Occupy energy levels called electron shells

- Those closest to the nucleus are most strongly attracted

- Each shell has distinct properties

- The # of electrons has an upper limit

- Shells closet to the nucleus fill first

Front 18

Bonding

Back 18

- involves interactions between electrons in their outer shell (valence shell)

- Full valence shells do not form bonds

Front 19

Inert Elements

Back 19

- Atoms are stable/inert when the outermost shell is complete.

- How to fill the atom's shell:

× Shell 1 can hold a max of 2 electrons

× Shell 2 can hold 8 electrons

× Shell 3 can hold 18 electrons

- Atoms will gain, lose, or share electrons to complete their outermost orbitals and reach a stable state.

Front 20

Rule of Eights

Back 20

Atoms are considered stable when their outermost orbital has 8 electrons; the exception is shell 1, which can only hold 2 electrons.

Front 21

Reactive Elements

Back 21

- Valence shells are not full and are unstable

- Tend to gain, lose, or share elements

- Allow for bond formation, which produces stable valence

Front 22

Ionic Bonds

Back 22

Form when electrons are completely transferred one atom to another

Front 23

Ions

Back 23

- Charged particles

- Anions are negative

- Cations are positive

- Either donate or accept electrons

Front 24

Covalent Bonds

Back 24

- Atoms become stable through shared electrons

- Single covalent bonds share one pair of electrons

- Double covalent bonds share two pairs of electrons

Front 25

Polarity

Back 25

- Covalently bonded molecules

× some are non-polar

× electrically neutral as a molecule

- Some are polar

× have a positive and negative side

Front 26

Hydrogen Bonds

Back 26

- Weak chemical bonds

- Hydrogen is attracted to the negative portion of polar molecules

- Provides attraction between molecules

Front 27

Synthesis Reaction

Back 27

A + B -> AB

- Atoms or molecules combine

- Energy is absorbed for bond formation

Front 28

Decomposition Reaction

Back 28

AB -> A + B

- Molecule is broken down

- Chemical energy is released

Front 29

Exchange Reaction

Back 29

AB + C -> AC + B

- Involves both synthesis and decomposition reactions

- Switch is the mode between molecule parts and different molecules are made

Front 30

Organic Compounds

Back 30

- Contain Carbon

- Most are covalently bonded

ex.: C6H12O6 (glucose)

Front 31

Inorganic Compounds

Back 31

- Lack Carbon

- Tend to be simpler compounds

ex.: H2O (water)

Front 32

Water

Back 32

- Most abundant inorganic compound

- Vital properties:

× High heat capacity

× Polarity/solvent properties

× Chemical reactivity

× Cushioning

Front 33

Salts

Back 33

- Easily dissociate into ions in the presence of water

- Vital to many bodily functions

- Include electrolytes which conduct electrical currents

Front 34

Atomic Mass

Back 34

the sum of the massed of all protons and neutrons contained in its nucleus

Front 35

Synthesis Reactions

Back 35

occur when two or more atoms molecules combine to form a larger, complex molecules