exam 1 Flashcards
Matter
Anything that takes up space and mass
Element
Substance that cannot be broken down to other substances by chemical reactions
Compound
Substance consisting of two or more different elements combined in a fixed ratio
Essential elements
20-25% of elements that an organsim needs to live a healthy life and reproduce
Trace elements
Required by an organism in only minute quantities
Atomic nucleus
Protons and neutrons Are packed together rightly in a dense core at the center of an atom
Dalton
Unit of measurement honor of john dalton
- the atomic mass is measured in Dalton’s and is roughly equal to the mass number
Atomic number
Number of protons
Mass number
Sum of protons and nuetrons
Atomic mass
Approximation of the total mass of an atom
Isotopes
Same protons different neutrons
Radioactive isotope
Nucleus decays spontaneously, giving off particles and energy
Half-life
Time it takes for 50%!+~ the parent isotope to decay
Rediometric dating
Scientist measure the ratio of different isotopes and calculator how many half lives have passed since an organsim im was fossilized or a rock was formed
Energy
Defined as the capacity to cause change
Potential energy
Energy that matter possesses because of it’s location or structure
Valence electrons
Outer electrons
Valence shell
Outermost electron shell
Chemical bonds
Atoms staying close together held by attractions
-strongest kinds of chemical bonds are covalent and ionic bonds
Covalent bond
The sharing of a pair of electrons by two atoms
Molecule
Two or more atoms held together by a covalent bonds
Single bond
A pair of shared electrons ( 1 line)
Double bond
Sharing two pairs of valence electrons
Electronegativity
The attraction of a particular atom for the electrons of a covalent bond
Non polar covalent bond
Electrons are shared equally because the tel atoms when the same Electronegativity
Polar covalent
Bonds vary in their polarity depending on the relative Electronegativity of the two atoms ( partial energy)
Ions
The two resulting oppositely charged atoms or molecules (stole electron)
Cation
Positively charged ion
Anion
Negatively charged ion
Ionic bond
Any two ions of opposite charge
Ionic compounds or salts
Compounds formed by ionic bonds
Van see waals interactions
Individually weak and occur only when atoms and molecules are very close together
Occur between transiently positive and negative regions of molecules
Chemical reactions
The making and breaking of chemical bonds,leading to changes in the composition of matter
Reactants and products
When we write a chemical reaction , we use an arrow to indicate the conversion of the starting materials called the reactants to the products
Hydrogen bond
An attraction between a hydrogen atom carrying a partial positive charge and an electronegative atom
Chemical reactants
Change reactants into products while conserving matter
Chemical equilibrium
Reached when the flawed and reserve reaction rates are equal
Cohesion
Water sticks to water
- make water more structured
- many molecules linked by multiple hydrogen bonds
Adhesion
The clinging of one substance to another
Surface tension
Measure of how difficult it is to stretch or break the surface of a liquid
-related to cohesion
Kinetic energy
The energy of motion
Thermal energy
The kinetic energy associated with the random movement of atoms or molecules
Temperature
Measure of energy that represents the average kinetic energy of the molecules in a body of matter, regardless of volume,where as the total thermal energy depends in part on the matters volume
Heat
Thermal energy in transfer from one body of matter to another
Calorie (cal)
One convienient unit of hear used in this book
Specific heat
The amount of heat that must be absorbed or lost for 1 g of that substance to change it’s temperature by 1C
Heat of vaporization
The quantity of heat a liquid must absorb for 1g of it to be converted from the liquid to the gaseous state.
Evaporating cooling
Occurs because the hottest molecules, those with the greatest kinetic energy, are the most likely to leave as gas.
Molecular mass
Sum of the masses of all the atoms in a molecule
Mole
Represents an exact number if objects 6.02X10^23 which is called Avogadro’s number
Molarity
The number of miles of solute per liter of solution is the unit of concentration most often used by bioloagist for aqueous solitons
Hydrogen ion
A single proton with a charge of 1+
Hydroxide Ion
Water molecule that lost a proton
-1 charge
Hydronium ion
The proton binds to the other water molecule
Base
A substance that reduces the hydrogen ion concentration of a solution
Buffer
Substance that minimizes changes in Thr concentrations of H+ and OH- in a solution
Ocean acidification
When CO2 dissolves in seawater, it reacts with water to from carbonic acid, which lowers ocean ph
Solution
A liquid that is a completely homogeneous mixture of two or more substances
Solvent
The dissolving agent of a solution
Solute
Substance that is dissolved
Aqueous solution
One in which the solute is dissolved in water ; water is the solvent
Hydrogen shell
The sphere of water molecules around each dissolved ion
Hydrophilic
Any substance that has an affinity for waster is said to by this
Emergent properties
Due to the arrangement and interactions of parts as complexity increases
System biology
The exploration of a biological system by analyzing the intersections along it’s parts
Eukaryotic cell
Contains membranes enclosed
Oraganells (bigger)
Prokaryotic
Lacks a nucleus or other membrane enclose organella
Gene
Each section do the DNA of a chomsome
Gene expression
The entire process by which the information in a gene directs the manufacture of a cellular product
Genome
The entire library of genetic instructions that an organism inherits
Bioinformatics
The use of computational tools to store, organize, and analyze the huge volume of data that results from high-throughput methods.
Bacteria
Diverse and widespread prokaryotics
Arches
Love in earths extream environments such as salty lakes boiling hot springs
Eukarya
Kingdom plantae, fungi, animal is and protist
Protists
Unicellular eukaryotes
Inquiry
A search for information and explanations of natural phenomena
Inductive reasoning
Generalizations from a large number of specific observations
Deductive reasoning
From general we extrapolate to the specific results
Variables
Both the factor that is manipulated and the effects that are measured are types of experimental variables , factors that vary in an experiment
Controlled experiment
Designed to compare an experimental group with a control group
Independent variable
Factor that is manipulated by the researcher
Dependent variable
Factor that is measured in the experiment
Theory
General enough topspin off many new specific hypothesis
Supported by greater body of evidence
Model organism
A species that is easy to grow in the lab and lends itself particularly well to the questions being investigated
The 5 themes
Organization Information Energy and matter Interactions Evolution
Hydrocarbons
Organic molecules consisting of only carbon and hydrogen
Isomers
Compounds that have the same number if atoms of the same elements but different structure and hence different properties.
Structural isomers
Differ in the covalent arrangements of their atoms
CIA-trams isomers (geometric)
Carbons have covalent bonds to the same atoms , but these atoms differ in their spatial arrangements did to the I flexibility of double bonds.
Enantiomers
Isomers that are mirror images of each other and that differ in shape due to the presence of an asymmetric Carbon, one that is attached to 4 different atoms or group of atoms.
Functional groups
Chemical groups are directly involve in chemical reactions
Adenosine triphosphate (ATP)
Organic molecule attached to a string of there phosphate groups
H30
Hydronium
Hydroxide
OH- ( lost proton)
