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Biology 12 > Chapter 1 - Review > Flashcards

Chapter 1 - Review Flashcards

0
Q

Elements

A

2 or more of the same type of atoms bonded together

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1
Q

Matter

A
  • anything that takes up space or weight
  • found in 3 phases: solid, liquid, gas
  • made up of elements
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2
Q

Atom

A

Smallest unit of matter

Ex. Carbon

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3
Q

Molecule

A

2 or more atoms bonded together (can be same type of atoms or different)
Ex. C2

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4
Q

Compound

A

2 or more different types of elements bonded together

Ex. H20

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5
Q

Sub-atomic particles

A
  • protons
  • neutrons
  • electrons
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6
Q

Protons

A
  • inside nucleus
  • positive charge
  • weigh 1 atomic mass unit
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7
Q

Neutrons

A
  • inside nucleus
  • no charge
  • weigh 1 atomic mass unit
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8
Q

Electrons

A
  • move around nucleus in orbitals
  • negative charge
  • weigh nothing
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9
Q

Atomic number

A

Number of protons (which is equal to the number of electrons)

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10
Q

Atomic mass

A

Number of protons and neutrons

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11
Q

Isotopes

A

Atoms of the same element with a different mass because they have a different number of neutrons
Ex. Carbon has 3 isotopes

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12
Q

Tracers

A

Radioactive isotopes used to follow biological processes/pathways in living organisms
Ex. Dye in bloodstream to check for clots

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13
Q

Heavy isotope

A

An atom with more neutrons

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14
Q

Which 4 elements are the most common in the human body?

A

Oxygen, carbon, hydrogen, nitrogen

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15
Q

Why does a neutral atom have no net charge?

A

Because the protons and electrons cancel each other out

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16
Q

What determines if an atom will gain, lose, or share electrons?

A

The number of electrons in its shell

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17
Q

As the number of neutrons increases, the atomic number _______ and the atomic mass ________

A
  • stays the same

- increases

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18
Q

How are electrons held in orbit?

A

By their attraction to protons

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19
Q

Octet rule

A
  • 1st orbit holds a maximum of 2 electrons

- the rest hold a maximum of 8

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20
Q

Why do atoms bond?

A

To create a stable outer unit

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21
Q

Chemical bonds

A

Form when electrons are gained, lost, or shared

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22
Q

Ionic bond

A
  • between metals & non-metals
  • electrons leave one atom and attach to the new atom
  • lose an e: positively charged ion
  • gain and e: negatively charged ion
  • ions are held together by a weak electromagnetic force
23
Q

Covalent bond

A
  • between 2 non-metals
  • electrons shared, not transferred
  • non-polar bond: electrons shared equally because atoms are similar in size
  • polar bond: difference in atom sizes causes one to have more pull on the shared election, resulting in a difference in charge between the 2 poles of the molecule (ex water)
24
Q

Hydrogen bond

A
  • gives structure to liquid water
  • stabilizes nucleic acids & other large molecules
  • drawn as a dotted line because they are so weak
25
Q

Electron-dot/Lewis dot formula

A
  • shows only the electrons in the outer orbital
  • electrons shown by dots
  • place 1 dot on each quadrant, then double up
26
Q

Structural formula

A
  • bonds shown by straight lines

- 1 line = 1 pair of shared electrons

27
Q

Molecular formula

A
  • shows only the amount of each type of atom in the molecule
  • does not indicate any bonds

Ex. CH4

28
Q

Empirical formula

A

Show lowest ratio of atoms (kind of like reducing the molecular formula)

Ex. C2H6 in molecular = CH3 in empirical

29
Q

More than 1 bond…

A
  • atoms may share more than just 1 pair of electrons
  • if 2 pairs are shared: double bond
  • if 3 pairs are shared: triple bond
  • double & triple bonds are much stronger than single bonds
30
Q

Chemical make-up of water

A
  • 2 hydrogen atoms joined to the oxygen atom by a single covalent bond
  • polar molecule
31
Q

Properties of water

A
  • cohesion
  • surface tension
  • specific heat
  • evaporative cooling
  • solvent/dissolving agent
32
Q

Cohesion

A

Water molecules are bonded together by hydrogen bonds, giving water more structure than most other liquids

33
Q

Surface tension

A

Water has a great surface tension - bugs and lizards can walk across it without breaking the surface tension

34
Q

Specific heat

A
  • Has high specific heat
    (1 calorie per gram per degree Celsius)
  • takes a long time to heat up due to the number of h-bonds
  • helps protect living systems from rapid temperature changes & maintain a normal internal environment
35
Q

Evaporative cooling

A

When the hottest molecules leave, the surface of the liquid that remains cools down

36
Q

Solvent

A
  • Water is a solvent/dissolving agent…aka an aqueous solution
  • can dissolve polar molecules (ex salt & sugar)
37
Q

Hydrophilic

A

A substance with an affinity to water

Ex. Cotton, which absorbs water

38
Q

Hydrophobic

A

A substance that repels water

Ex. Oil

39
Q

Water in the human body

A
  • human body is approximately 65% water

- as you get older, the amount of water reduces

40
Q

Effects of dehydration

A
  • fuzzy short-term memory
  • trouble with basic math
  • problems focusing on small print
41
Q

Water’s uses in the body

A
  • lubricant
  • base for saliva
  • forms fluids surrounding joints
  • regulates body temperature
  • prevents constipation
  • regulates metabolism
42
Q

Dissociation

A

Water molecules dissociate (break apart) to produce hydrogen ions (H+) and hydroxide ions (OH-)

43
Q

How to determine acidity vs bascity

A

Determined by number of free H or OH ions

44
Q

Acids

A

Molecules that dissociate in water to release H

45
Q

Bases

A

Either take up H or release OH

46
Q

Oxidized

A

When an atom loses an electron or when a molecule loses a hydrogen atom

47
Q

Reduced

A

When an atom gains an electron or molecule gains a hydrogen atom

48
Q

pH

A
  • indicates acidity/basicity of a solution
  • scale ranges from 0-14
  • each step up or down the scale is equal to a jump in 10x the strength

Ex. Acid of pH 4 is 100x stronger than acid of pH 6

49
Q

Biological importance of pH regulation

A

metabolic reactions, molecular structure, and toxicity of molecules depend on pH

50
Q

Neutralization

A
  • When an equally strong acid & base react
  • produces water & salt

Ex. HCl + NaOH –> NaCl + H2O

51
Q

Buffers

A

Chemicals that resist pH changes by taking up excess H or OH

Ex. Buffering of blood by carbonic acid & bicarbonate ion
When hydrogen is added to blood:
H + HCO3 –> H2CO3

52
Q

Buffering blood with hydroxide ions

A

Water is formed

Ex. **OH + H2CO3 –> HCO3 + H2O

53
Q

If a buffer is added to an acidic solution, the pH will ______

A

Increase

54
Q

If a buffer is added to a basic solution, the pH will ________

A

Decrease

Biology 12 (14 decks)

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