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Chapter 2 - Bio 111
Test 1
82
Biology
Undergraduate 3
09/22/2013

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Term
What is all matter composed of?
Definition
Atoms.
Term
What are 2 characteristics of matter?
Definition
1.) Has mass
2.) Occupies space
Term
What are the 3 components of atoms?
Definition
1.) Protons
2.) Neutrons
3.) Electrons
Term
What are the relative masses of protons, neutrons, and electrons?
Definition
Protons and neutrons have roughly the same mass where electrons have a much smaller mass
Term
What makes up an atomic number?
Definition
THE NUMBER OF PROTONS
Term
Atoms with the same atomic number have the same chemical properties and belong to the same ___________.
Definition
element
Term
What is mass?
Definition
The amount of something
Term
What is weight?
Definition
The force of gravity exerted on something. It is mass in the concept of gravity.
Term
What makes up atomic mass?
Definition
The sum of protons and neutrons
Term
What is an isotope?
Definition
Same # of protons, different number of neutrons.
Term
Radioactive isotopes are what?
Definition
Unstable and emit radiation as the nucleus breaks up.
Term
What do we use radioactive isotopes for?
Definition
Carbon 14 dating.
Term
What is a half-life?
Definition
The time it takes for one-half of the atoms in a sample to decay.
Term
What are electrons?
Definition
Negatively charged particles with very small mass
Term
What is a neutral atom?
Definition
Same # of protons and electrons
Term
What is an ion?
Definition
A charged atom. Different number of protons and electrons
Term
What is a cation?
Definition
Fewer electrons than protons. Positively charged.
Term
What is an anion?
Definition
Have more electrons than protons. Negatively charged.
Term
Are cations usualy oxidized of reduced?
Definition
Oxidized, easier to lose than to gain.
Term
Are anions usually oxidized or reduced?
Definition
Reduced, easier to gain than to lose.
Term
What are orbitals?
Definition
where we can predict the location of an electron
Term
What does electron arrangement effect?
Definition
Atom's chemical behavior
Term
How many electrons can each orbital contain?
Definition
2
Term
What do electrons posses? How does their location effect this?
Definition
Potential energy. Further from nucleus, more energy.
Term
Energy LEVELS are different from energy ORBITALS how?
Definition
Levels = energy
Orbital = location
Term
Electrons can be transferred from one atom to another while retaining what?
Definition
Their energy
Term
What is oxidation?
Definition
Loss
Term
What is reduction?
Definition
Gain
Term
How do periodic tables display elements?
Definition
According to valence electrons
Term
What is a valence electron?
Definition
Number of electrons in outermost energy level.
Term
Non reactive elements have how many valence electrons?
Definition
8
Term
What is the octet rule?
Definition
Completely full outer energy levels. (8)
Term
How many naturally occurring elements are there?
Definition
90
Term
How many elements are found in living organisms?
Definition
12
Term
What 4 elements make up 96.3% of human body weight?
Definition
Carbon, Hydrogen, Oxygen, and Nitrogen
Term
What make up organic molecules?
Definition
CHON
Term
Atoms with full energy levels are less or more reactive than those with unfilled energy levels?
Definition
Less reactive
Term
What are molecules?
Definition
Groups of atoms held together in a stable association.
Term
What are compounds?
Definition
Molecules containing more than one type of element
Term
What are atoms held together by?
Definition
Chemical bonds.
Term
What are ionic bonds?
Definition
Electrostatic interations between 2 molecules that can be disrupted by electrical attraction with water molecules.
Term
Which is stronger: ionic or covalent?
Definition
Covalent
Term
What is a covalent bond?
Definition
Form when atoms share 2 of more PAIRS of valence electrons.
Term
Is there a charge with covalent bonds?
Definition
No, no net charge, satifies octet, no unpaired electrons.
Term
What is the strength of a covalent bond dependent on?
Definition
The number of shared electrons.
Term
What do chemical reactions involve?
Definition
The formation or breaking of chemical bonds.
Term
What are reactants?
Definition
The original molecule in a reaction
Term
What are the products?
Definition
Molecules resulting from a reaction.
Term
6 H20 + 6 CO2 -> C6H12O6 + 6 O2 is what?
Definition
Photosynthesis. The product is glucose.
Term
What influences chemical reactions?
Definition
1. Temperature
2. Concentration of reactants to products
3. Catalysts
Term
Electronegativity is an atom's what?
Definition
Affinity for electrons. How greedy an atom is for electrons in the structure of a covalent bond.
Term
What does differences in EN dictate?
Definition
How electrons are distributed in a covalent bond
Term
Nonpolar covalent bonds have unequal or equal sharing of electrons?
Definition
Equal
Term
Polar covalent bonds have unequal or equal sharing of electrons?
Definition
Unequal
Term
In a nonpolar covalent bond, where are the electrons located?
Definition
In the center
Term
In a polar covalent bond, where are electrons located?
Definition
They are closer to the element with the higher EN
Term
What is the EN level for Oxygen?
Definition
3.5
Term
What is the EN level for Nitrogen?
Definition
3.0
Term
What is the EN level for Carbon?
Definition
2.5
Term
What is the En level for Hydrogen?
Definition
2.1
Term
What is an important characteristic of water?
Definition
Hydrogen bonding
Term
Which bonds in H2O are highly polar?
Definition
the bonds between hydrogen and oxygen
Term
Oxygen is partially _______ while hydrogen is partially ________.
Definition
Negative/positive
Term
Are water molecules polar or nonpolar?
Definition
Polar
Term
What is a hydrogen bond?
Definition
A weak attraction between the partially negative oxygen of one water molecule and the partially positive hydrogen molecule of a DIFFERENT water molecule.
Term
What can hydrogen bonds form between?
Definition
1.) Between water molecules
2.) Between water and another charged molecule
Term
What is cohesion?
Definition
Water molecules sticking to each other by hydrogen bonds. Causes surface tension. Only occurs with other water molecules.
Term
What is adhesion?
Definition
Water molecules sticking to other polar molecules by hydrogen bonding. Can be water, can be just another polar molecule.
Term
What are 6 properties of water?
Definition
1.) Has high specific heat which requires a large amount of energy. This is so other organisms do not boil.

2.) Water has a high heat of vaporizing. The evaporating of water form a surface causes cooling of a surface. Sweating.

3.) Solid water is less dense than liquid water. Ice floating in drinks

4.) Water is a good solvent because is dissolves polar molecules and ions. Universal solvent.

5.) Water organizes nonpolar molecules. Hydrophilic = water loving. Hydrophobic = water fearing. Water causes hydrophobic molecules to assume specific shapes.

6.) Water can form/break apart into ions.
H2O -> OH- + H+
Term
What do water molecules aggregate around?
Definition
It's respective charge. Postive aggregates around negative and vice versa.
Term
What is the neutral pH?
Definition
7
Term
If pH is above 7 it is?
Definition
Basic
Term
If pH is below 7 it is?
Definition
Acidic
Term
pH is the negative logarithm what?
Definition
-log[H+]
Term
What is an acid?
Definition
Any substance that disassociates in water to increase the H+ concentration/lowers pH
Term
The stronger the acid, the more _______ it produces
Definition
H+ ions
Term
What is a base?
Definition
A substance that combines with H+ in water and lowers the H+ concentration.
Term
What is a buffer?
Definition
Any substance that resists changes in pH
Term
How does a buffer act when a base is added?
Definition
Releases H+ ions, raising the pH
Term
How does a buffer act when an acid is added?
Definition
Absorbing H+ ions, lowers the pH
Term
What does the range of effectiveness depend on?
Definition
Particular types of buffers
Term
What do most biological buffers consist of?
Definition
A pair of molecules; one acid and one base.
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