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Chapter 2
AP
42
Biology
Undergraduate 1
02/11/2014

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Term
Matter
Definition
anything that has mass and occupies space
Term
3 states of matter
Definition
Solid- definite shape and volume
Liquid - changeable shape; def volume
Gas - changeable shape and volume
Term
Energy
Definition
Capacity to do work or put matter into motion
Term
Kinetic Energy
Definition
energy in action
Term
Potential Energy
Definition
stored (inactive) energy
Term
Chemical Energy
Definition
Stored in bonds of chemical substances
Term
Electrical Energy
Definition
Results from movement of charged particles
Term
Mechanical Energy
Definition
Directly involved in moving matter
Term
Radiant/Electromagnetic Energy
Definition
Travels in waves (eg visible light, ultraviolet light, and x-rays)
Term
Elements
Definition
Matter is composed of elements

Elements cannot be broken into simpler substances by ordinary chemical methods

Each has unique properties
Physical
Detectable with our senses, or are measurable
Chemical
how atoms interact (bond w/ one another)
Term
Atoms
Definition
Unique building block for each element

Give each element its physical and chem properties

Smallest particles of an element with properties of that element
Term
Major Elements of the Human Body
Definition
Carbon, Hydrogen, Oxygen, Nitrogen
Term
Subatomic Particles
Definition
Proton, Neutrons, Electrons
Term
Atomic number
Definition
Number of protons in nucleus

subscript to left of atomic symbol.

3(bot)Li
Term
Mass number
Definition
Total number of protons and neutrons in nucleus

Written as superscript to left of atomic symbol (7top)Li
Term
Isotopes
Definition
Structural variations of atoms

Differ in the number of neutrons they contain

Atomic number same; mass numbers different
Term
Atomic weight
Definition
Average of mass numbers (relative weights) of all isotopes of an atom
Term
Radioisotopes
Definition
Heavy isotopes decompose to more stable forms
Spontaneous decay called radioactivity

Can be detected with scanners

All damage living tissues
Some used to destroy localized cancer
Term
Molecule
Definition
Two or more atoms bonded together

Smallest particle of a compound with specific characteristics of the compound
Term
Molecule
Definition
Two or more atoms bonded together

Smallest particle of a compound with specific characteristics of the compound
Term
Compound
Definition
Two or more different kinds of atoms bonded together
Term
Mixtures (3 types)
Definition
Solutions, Colloids, Suspension
Term
Solutions
Definition
Homogenous mixture

Solute particles are very tiny, do not settle out or scatter light

Solvent
Substance present in greatest (water)
Solute
present in smaller ammounts
Term
Concentration of True Solutions
Definition
Can be expressed as
Percent of solute in total solution (assumed to be water)
Parts solute per 100 parts solvent
Milligrams per deciliter (mg/dl)
Molarity, or moles per liter (M)
1 mole of an element or compound = Its atomic or molecular weight (sum of atomic weights) in grams
1 mole of any substance contains 6.02  1023 molecules of that substance (Avogadro’s number)
Term
Colloids (emulsions)
Definition
Heterogenous mixtures

Solute particles are larger than in a solution and scatter light; do not settle out

Large solute particles do not settle out

Some undergo sol-gel transformations
Term
Suspensions
Definition
Heterogeneous mixtures

Solute particles are very large; and may scatter light

Large visible solutes settle out
Term
Mixtures
Definition
No chemical bonding between components

Can be separated by physical means, such as straining or filtering

Heterogenous or homogenous
Term
Compounds
Definition
Chemical bonding between components

Can be separated only by breaking bonds

All homogenous
Term
Chemical Bonds
Definition
energy relationships between electrons of reacting atoms

Electrons can occupy up to seven electron shells around nucleus

Electrons in valence shell (outermost electron shell)
Have most potential energy
Are chemically reactive electrons
Octet rule
Except for the first shell (2 E max) atoms interact to have eight electrons in their valence shell
Term
Chemically Inert Elements
Definition
Stable and unreactive

Valence shell fully occupied or contains eight electrons

Noble gases
Term
Chemically Reactive Elements
Definition
Valance shell not full

Tend to gain, lose, or share electrons with other atoms to achieve stability
Term
Three major Chemical Bonds
Definition
Ionic, Covalent, Hydrogen
Term
Ionic Bonds
Definition
Ions
Atoms gain or lose electrons and become charged (#P =/ #E)

Transfer of valence shell electrons from one atom to another forms ions
One become an anion (- charge)
Atom gained one or more E
One become cation
Atom lost one or more E
Attraction of opposite charges results in an ionic bond
Term
Covalent Bonds
Definition
Formed by sharing of two or more valence shell electrons

Allows each atom to fill its valence shell at least part of the time
Term
Nonpolar Covalent Bonds
Definition
Electrons shared equally
Produced electrically balanced, nonpolar moles such as CO2
Term
Polar Covalent Bonds
Definition
Unequal sharing of electrons produces polar (AKA dipole) molecules such as H2O
Atoms in bond have different electron-attracting abilities

Small atoms with six or seven valence electrons are electronegative,
strong electron-attracting abil (O)

Most atoms with one or two valence shell electros are electropositive, (sodiumn)
Term
Hydrogen Bonds
Definition
Attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule
Not true bond
common between dipoles such as water
Also act as intramolecular bonds, holding a large molecule in 3d shape
Term
Patterns of Chemical Reactions
Definition
Synthesis, Decomposition, Exchange
Term
Synthesis Reactions
Definition
A + B =AB
Atoms or molecules combine to form larger, more complex molecule
Always involve bond formation
Anabolic
Term
Decomposition Reaction
Definition
AB -> A + B

Molecule is broken down into smaller ones

Involve breaking of bonds
Catabolic
Term
Exchange Reactions
Definition
AB + C -> AC + B
Also called displacement reactions
Involve both synthesis and decomposition
Bonds are both made and broken
Term
oxidation-reduction reactions
Definition
Are decomposition reactions
Reactions in whihc food fuels are broken down for energy

Are also exchange reactions because electrons are exchanged between reactants
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