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AP Bio > essential chem (1-18) > Flashcards

essential chem (1-18) Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

contrast the term element with compound: an element is a … substance composed of …. that cannot be …. whereas a compound is composed of … and can be …

A

pure; one type of atom; broken down; two or more elements; broken down

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2
Q

(symbols and charges) carbon

A

C; 4-

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3
Q

(symbols and charges) hydrogen

A

H; 1+

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4
Q

(symbols and charges) oxygen

A

O; 2-

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5
Q

(symbols and charges) nitrogen

A

N; 3-

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6
Q

(symbols and charges) phosphorus

A

P; 3-

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7
Q

(symbols and charges) sulfur

A

S; 2-

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8
Q

nucleus: small … region in … of atom

A

positively charged; center

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9
Q

proton: …. charged atomic particle, located in …

A

positively; nucleus

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10
Q

neutron: electrically … particle in atomic …

A

neutral; nucleus

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11
Q

electron: …. charged particle located in …. that surround the …

A

negatively; orbitals; nucleus

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12
Q

electron density: region of …. where electron is located

A

probability

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13
Q

(contrast the atomic mass and atomic number) Atomic mass is the mass of a single … of an element that is nearly equivalent to the total number of …. and … in the nucleus, whereas the atomic number is the number of … in an atom

A

isotope; protons; neutrons; protons

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14
Q

(what is the difference between the terms atomic mass and atomic weight) atomic weight takes into consideration the masses of …. where the atomic mass does not

A

all the isotopes of an element

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15
Q

(what is an isotope and what is “special” about radioactive isotopes) an isotope is an atom of an element that contains a different number of …. radioactive isotopes have …. due to an unfavorable ratio of …. For radioactive isotopes, the … changes and the isotopes … into a different …

A

neutrons; unstable nuclei; nucleic particles; atomic mass; decay; form

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16
Q

(what determines interactions between atoms? why are valence electrons important?) interactions are determined by the number of ….. They are important because they are the electrons through which …. are formed, and they determine if an element acts as a … or an …

A

valence electrons; chemical bonds; cation; anion

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17
Q

chemical bond: an … between atoms entailing the sharing or taking of …. that … atoms together

A

attraction; valence electrons; binds

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18
Q

covalent bond: a bond in which atoms … electrons

A

share

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19
Q

single bond: a bond in which … of electrons are shared between atoms

A

one pair

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20
Q

double bond: a bond in which … of electrons are shared between atoms

A

two pairs

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21
Q

electronegativity: the ability of an atom to … the electrons of an …

A

attract; adjacent atom

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22
Q

nonpolar covalent bond: a covalent bond in which electrons are shared …

A

equally

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23
Q

polar covalent bond: a covalent bond in which electrons are shared … due to differing …. of the bonding atoms

A

unequally; electronegativities

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24
Q

(what is the difference between a structural and molecular formula) a structural formula indicates the … of bonds and the … of a molecule’s atoms through the use of …. A molecular formula, however, gives information concerning the … and … of atoms in a molecule

A

number; arrangement; dashes; numbers; types

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25
Q

oxygen gas

A

O2

26
Q

Carbon dioxide

A

CO2

27
Q

glucose

A

C6H12O6

28
Q

phosphate

A

PO4 3-

29
Q

Ammonia

A

NH3

30
Q

Water

A

H2O

31
Q

(How do ionic bonds compare with covalent bonds) an ionic bond occurs due to … between positively and negatively charged ions and entails the … and … of electrons. Howeer, covalent bonding merely entails the …. of electrons

A

electrostatic; loss; gain; sharing

32
Q

(compare and contrast hydrogen bonds and van der Waals interactions) hydrogen bonds are stronger intermolecular forces that occur when hydrogen is bonded with a highly …. and then bonds with another on an ….. Van der Waals forces, however, are weaker and are based on …. that can, in some cases, occur in all molecules (e.g.. ….)

A

electronegative atom; adjacent molecule; dipoles; induced dipoles

33
Q

(dynamic chemical equilibrium) dynamic chemical equilibrium is a state in which the rate at which products are formed is equal to the rate at which

A

the reverse reaction occurs, where the products reform reactants

34
Q

water is polar due to the presence of … that results from the … of electrons located on the oxygen atom

A

dipoles; lone pairs

35
Q

(property and relation to water) cohesion: a molecule’s attraction toward molecules of the ….
cohesion in water occurs due to the fact that water molecules undergo …, which are strong intermolecular forces. through hydrogen bonding, the positively charged hydrogens on one water molecule bond with the …. on adjacent water molecules

A

same identity; hydrogen bonding; negatively charged oxygens

36
Q

(property and relation to water) adhesion: a molecule’s attraction toward particles of a … The hydrogens on water bond …. on an adjacent molecule and the oxygen bonds with a ….

A

different substance; with negatively charged ions; positively charged ion

37
Q

(property and relation to water) surface tension: phenomenon through which … forces cause a liquid to adopt a …. so as to minimize …. Measures the energy required to increase a liquid’s …
surface tension in water occurs as a result of hydrogen bonding. the molecule’s at the water’s surface are …. to those below it, resulting in the spherical shape

A

cohesive; spherical; surface area; surface area; unequally attracted

38
Q

(property and relation to water) high specific heat: large amount of heat needed to raise the temperature of a … sample of a material by … The heat absorbed by water molecules is utilized as an …. to break the bonds and eventually increase the kinetic energy of the water molecules sufficiently so that they change state. however, due to the strength of water’s hydrogen bonds, a …. is necessary to … the bonds. Consequently, water tends to be more … to temperature changes and thus has a high specific heat

A

1 g; 1 K; energy source; large amount of heat; break; resistant

39
Q

(property and relation to water) heat of vaporization: amount of heat required for a liquid to …

A

become a gas

40
Q

(property and relation to water) evaporative cooling: process by which the evaporation of a liquid …
when water vaporizes, it makes use of the … that is available in its surroundings. it … this heat, which resultls in a lowered …

A

lowers temperatures; energy as heat; absorbs; atmospheric temperature

41
Q

(what is special about water and density) contrary to most substances, water is … dense in the solid state than in the liquid state

A

less

42
Q

(phenomena and properties of water) during the winter, air temperatures in the northern United States can remain below 0 degrees C for months, however animals in the lake survive:

A

ice less dense than water; high specific heat

43
Q

(phenomena and properties of water) many substances–for example, salt and sucrose,— dissolve quickly in water

A

polarity; water as “universal solvent”

44
Q

(phenomena and properties of water) when you pour water into a 25-ml graduated cylinder, a meniscus forms

A

adhesion

45
Q

(phenomena and properties of water) sweating and the evaporation of sweat from the body surfacing helping to reduce a human’s body temp

A

evaporative cooling

46
Q

(phenomena and properties of water) water drops that fall on a surface tend to form rounded drops or beads

A

cohesion and surface tension

47
Q

(phenomena and properties of water) water drops that fall on your car tend to bead or round up more after polishing

A

stronger cohesive forces indicate hydrophobic polish

48
Q

(phenomena and properties of water) if you touch the edge of a paper towel to a drop of colored water, the water will move up into (or be absorbed by) the towel

A

adhesion, capillary action

49
Q

solute: substance that

A

dissolves

50
Q

solvent

A

dissolving medium

51
Q

aqueous solution: a solution consisting of a substance

A

dissolved in water

52
Q

hydrophilic:

A

favors and interacts with water

53
Q

hydrophobic

A

repels water

54
Q

molarity: measure of ….; … solute/ … solution

A

concentration; moles; liters

55
Q

hydroxyl causes organic compounds to be more …, forms … bond and is …., present in … and some …

A

soluble; hydrogen; polar; sugars; amino acids

56
Q

carbonyl: increases …., …, present in …

A

melting/boiling pts; polar; sugars

57
Q

carboxyl: …, acts as an … and is present in a large number of …. molecules including … and …

A

charged; acid; biological; fatty acids; amino acids

58
Q

amino: acts as a …, …, included in … which form …

A

base; charged; amino acids; proteins

59
Q

sulfhydrl: aid in …, … present in some …, forms … bonds

A

stabilizing proteins; polar; amino acids; disulfide

60
Q

phosphate: …, acts as an …., capable of transferring … between .. molecules, ….

A

charged; aacid; energy; organic; polar

61
Q

(functional groups) when a functional group attaches to a …, it changes some …, determines the … and … a molecule will undergo

A

hydrocarbon; properties; polarity; type of reaction

AP Bio (32 decks)

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