Bio 1210 Week 1 Day 1

Front 1

Macromolecules

Back 1

are very large molecules formed by smaller molecules

Front 2

Monomers

Back 2

are individual units of a larger molecule

Front 3

Polymers

Back 3

are made up of monomer units bonded together

Front 4

Cell membranes are made up of

Back 4

Phospholipids

Front 5

All cell membranes are ____ they have a ____

Back 5

Bilipids. Bilayer

Front 6

What are the two sides to a cell membrane?

Back 6

hydrophilic- likes water, hydrophobic- doesnt like water

Front 7

Cell membranes seperate what?

Back 7

The inside and outside of a cell

Front 8

Unsaturated fats have:

Back 8

1 or more double bonds

Front 9

Polyunsaturated fats have:

Back 9

2 or more double bonds

Front 10

Saturated fats have:

Back 10

no double bonds.

Front 11

The plasma membrane separates ___ and _____

Back 11

living cells and non living surroundings

Front 12

The plasma membrane exhibits:

Back 12

selective permeability, allows some substances to cross, some not.

Front 13

The most abundant lipid in the plasma membrane are:

Back 13

Phospholipids

Front 14

The plasma membrane is made up of _____ heads and _____ tails

Back 14

phosphate heads (hydrophilic) and fatty acid tails (hydrophobic)

Front 15

Define matter

Back 15

any substance that takes up space and has mass

Front 16

what is matter made up of?

Back 16

elements

Front 17

what are the four major elements matter is made up of?

Back 17

carbon nitrogen hydrogen oxygen

Front 18

Define a compound

Back 18

a substance consisting of 2 or more different elements in a fixed ratio

Front 19

define a molecule

Back 19

is a combination of 2 or more elements.

Front 20

what is H2 and H20 examples of?

Back 20

H2 is a molecule but not a compound, H20 is both a compound and molecule

Front 21

What do elements consist of?

Back 21

a certain kind of atom that is different

Front 22

what are atoms composed of?

Back 22

3 subatomic particles: protons, neutrons, electrons

Front 23

how do elements relate to other elements in subatomic particles?

Back 23

they differ in number of subatomic particles.

Front 24

what do the number of protons define about an element?

Back 24

they define the element and atomic number

Front 25

what is an atomic mass?

Back 25

the sum of number of protons and neutrons in that atom.

Front 26

what is the difference between outer and inner orbitals of atoms?

Back 26

more energy absorbed outer orbital, energy is lost in inner orbital

Front 27

what is an orbital?

Back 27

the 3 dimensional space where electrons are found 90% of the time

Front 28

what are valence electrons?

Back 28

electrons found in the outer most shells or atoms

Front 29

what do atoms sometimes do to bonds?

Back 29

sometimes ships away electrons

Front 30

what is an ion?

Back 30

an atom with a charge

Front 31

what is an anion

Back 31

an ion with a negative charge

Front 32

what is a cation?

Back 32

an ion with a positive charge

Front 33

what is an ionic bond?

Back 33

the attraction between positive and negative ions

Front 34

what happens to an atom when it gains an electron?

Back 34

becomes negative

Front 35

what happens to an atom when it loses an electron?

Back 35

becomes positive

Front 36

what are covalent bonds

Back 36

the sharing of valence electrons

Front 37

what do covalent bonds do with electrons?

Back 37

share but do not strip away

Front 38

what is a single bond?

Back 38

when atoms share 1 electron

Front 39

what is a double covalent bond?

Back 39

when atoms share 2 electrons

Front 40

how many electrons are in a pair and double pair of electrons?

Back 40

2 and 4

Front 41

in a molecule with a more electronegative atom. what does the electronegative atom do?

Back 41

pulls shared electrons toward the more electronegative atom

Front 42

what is a non polar covalent bond?

Back 42

a covalent bond with the same pull. they share the electron equally.

Front 43

what is an example of a partial negative atom in a compound?

Back 43

Oxygen in h2o

Front 44

what is an example of a partial positive atom?

Back 44

Hydrogen in H2O

Front 45

what is a hydrogen bond?

Back 45

when a hydrogen atom attached to an electronegative atom is also attracted to another electronegative atom.

Front 46

how many hydrogen bonds can a watermolecule form?

Back 46

up to 4

Front 47

what type of molecule is water?

Back 47

a polar molecule.

Front 48

what is a polar molecule?

Back 48

atoms that are negatively charged and positively charged that attract eachother

Front 49

how does water stabilize air temperature?

Back 49

it absorbs heat from air and releases stored heat to air that is cooler.

Front 50

what is specific heat?

Back 50

the heat required to raise the temperature of 1g of substance by 1 degree

Front 51

what does ice do to water temperature?

Back 51

it protects it

Front 52

compare ice with water

Back 52

ice is more ordered and less dense

Front 53

what is a solute?

Back 53

a solid material that is dissolved in a solvent

Front 54

what is a solvent?

Back 54

the liquid substance that the solute dissolves in

Front 55

what is a solution?

Back 55

the homogenous mixture of a solvent and solute

Front 56

what does homogenous mean?

Back 56

the solute is fully dissolved and equally distributed

Front 57

what is hydrophilic and give an example of one

Back 57

has an affinity for water, ethanol

Front 58

what is hydrophobic and give an example of one

Back 58

has no affinity for water, fats

Front 59

is hydrophobic polar or non polar?

Back 59

non polar

Front 60

is hydrophilic polar or non polar?

Back 60

polar

Front 61

describe inorganic molecules

Back 61

simple, small and cannot perform complex functions

Front 62

describe organic molecules

Back 62

larger, more complex, and can carry energy necessary for metabolism

Front 63

name some examples of inorganic molecules

Back 63

salts, acids, bases

Front 64

name some examples of organic molecules

Back 64

carbs, lipids, protein, DNA

Front 65

name 4 organic compounds and their symbols

Back 65

Hydroxyl OH-, carboxyl COOH, amino NH-2, phosphate PO-4

Front 66

Atoms with an incomplete valence shell are:

Back 66

Chemically reactive.

Front 67

what is the bonding capacity of an atom in its first and valence shell?

Back 67

2 and 8.

Front 68

if an atom has 5 valence electrons, how many covalent bonds can this atom form?

Back 68

up to 3

Front 69

what is cohesion?

Back 69

the transport of water against gravity in plants through a network of water conducting cells

Front 70

what is adhesion?

Back 70

the counter of the downward pull of gravity by hydrogen bonds to the molecules of cell walls

Front 71

why are carbon atoms versatile?

Back 71

because they can form single, double, and triple bonds. it can also form 4 single bonds, it can form chains, branched chains and rings when connected to other carbon atoms.

Front 72

Why is carbon important?

Back 72

because its so versatile i can form bonds with other carbon molecules that serves as the basic structural component or "backbone" of macromolecules

Front 73

What are the major functional groups found in biomolecules and what are their charges?

Back 73

Hydroxyl - OH-

Carboxyl - COOH

Amino - NH-2

Phosphate PO-4

Front 74

Define and describe the formation of an ionic bond and covalent bond.

Back 74

An ionic bond is when opposite ion charges transfer valence electrons to eachother completely. A covalent bond is the sharing one or more electron pairs that hold them together.