Ch 2 - Life Chemistry and Energy Flashcards

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1
Q

pure substance that contains only one kind of atom

A

element

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2
Q

Which elements make up about 96% of all living matter?

A

Carbon
Hydrogen
Nitrogen
Oxygen

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3
Q

What determines how atoms with behave, and whether they will form bonds?

A

the electrons in the atom’s valence shell

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4
Q

Bonds that form when atoms gain or lose one or more electrons to achieve stability.

A

ionic bonds

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5
Q

The strong bonds that form when atoms share electrons.

A

covalent

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6
Q

Groups of atoms that give important properties to biological molecules.

A

Functional Groups

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7
Q

electrically charged particle that forms when an atom gains or loses one or more elections

A

ion
(cations + charged)
(anions - charged)

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8
Q

the attractive force that an atomic nucleus exerts on electrons in a covalent bond

A

electronegativity

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9
Q

if two atoms are close to each other in electronegativity, they will form what type of bond?

A

nonpolar covalent bond

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10
Q

when electrons are drawn to one nucleus more than the other, they will form what type of bond?

A

polar covalent bond

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11
Q

What explains the fact that water molecules are “sticky?”

A

Hydrogen Bonding

+H is attracted to -O

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12
Q

Water characteristic explained by Hydrogen bonding between water molecules.

A

Cohesion
(water is “sticky”)
(explains “surface tension”)

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13
Q

Water characteristic explained by Hydrogen bonding between water molecules and other substances.

A

Adhesion
(explains capillary action in plants)
(meniscus in graduate cylinder)
(water “climbs” up paper towel)

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14
Q

Explain why water makes an excellent solvent.

A

Polarity
Water is a polar molecule. Polar water molecules surround + and - ions (in Ionic compounds) as well as other polar molecules.

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15
Q

Substances that have an attraction to water

A

hydrophilic

polar molecules

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16
Q

Substances that don’t have an attraction to water

A

hydrophobic

non-polar molecules

17
Q

Why does ice float?

A

Hydrogen bonding in ice becomes stable, causing water to become less dense than liquid water. (H bonds in liquid water are constantly breaking and reforming)

18
Q

Water characteristic that resists changes in temperature.

A

High specific heat

water must absorb a lot of energy to break H bonds before it will change temperature!

19
Q

Water characteristic that explains the difficulty in changing liquid water into its gaseous form.

A

Heat of Vaporization
(water must absorb a lot of energy to break H bonds - it absorbs this energy from its surroundings and thus has a cooling effect on its surroundings)

20
Q

Describes how acidic or basic a solutions is

A

pH

21
Q

H+ = OH-

A
neutral solution  
(pH = 7)
22
Q

H+ > OH-

A

acidic solution

pH < 7

23
Q

H+ < OH-

A

basic solution

pH > 7

24
Q

Why must the pH of living cells be about 7?

A

pH affects the shape of molecules - altered pH will affect the function of molecules and therefore affect cellular function

25
Q

chemical reactions that build larger molecules from smaller molecules

A

dehydration synthesis
(water taken out)
(energy input)
(anabolic reactions)

26
Q

chemical reactions that split larger molecules into smaller molecules

A

hydrolysis
(water input)
(energy released)
(catabolic reactions)

27
Q

chemical reaction that require input of energy

A

endergonic (endothermic)

anabolic reactions

28
Q

chemical reaction that release energy stored in bonds

A

exergonic (exothermic)

catabolic reactions

29
Q

1st law of thermodynamics

A

energy is neither created nor destroyed

total energy before and after energy conversion in a reaction is the same

30
Q

2nd law of thermodynamics

A

disorder tends to increase
(Entropy is increased)
(some energy becomes unavailable for doing work)

31
Q

measure of the disorder in a system

A

entropy