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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
Hydrogen bond
- gives structure to liquid water - stabilizes nucleic acids & other large molecules - drawn as a dotted line because they are so weak
25
Electron-dot/Lewis dot formula
- shows only the electrons in the outer orbital - electrons shown by dots - place 1 dot on each quadrant, then double up
26
Structural formula
- bonds shown by straight lines | - 1 line = 1 pair of shared electrons
27
Molecular formula
- shows only the amount of each type of atom in the molecule - does not indicate any bonds Ex. CH4
28
Empirical formula
Show lowest ratio of atoms (kind of like reducing the molecular formula) Ex. C2H6 in molecular = CH3 in empirical
29
More than 1 bond...
- 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
Chemical make-up of water
- 2 hydrogen atoms joined to the oxygen atom by a single covalent bond - polar molecule
31
Properties of water
- cohesion - surface tension - specific heat - evaporative cooling - solvent/dissolving agent
32
Cohesion
Water molecules are bonded together by hydrogen bonds, giving water more structure than most other liquids
33
Surface tension
Water has a great surface tension - bugs and lizards can walk across it without breaking the surface tension
34
Specific heat
- 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
Evaporative cooling
When the hottest molecules leave, the surface of the liquid that remains cools down
36
Solvent
- Water is a solvent/dissolving agent...aka an aqueous solution - can dissolve polar molecules (ex salt & sugar)
37
Hydrophilic
A substance with an affinity to water | Ex. Cotton, which absorbs water
38
Hydrophobic
A substance that repels water | Ex. Oil
39
Water in the human body
- human body is approximately 65% water | - as you get older, the amount of water reduces
40
Effects of dehydration
- fuzzy short-term memory - trouble with basic math - problems focusing on small print
41
Water's uses in the body
- lubricant - base for saliva - forms fluids surrounding joints - regulates body temperature - prevents constipation - regulates metabolism
42
Dissociation
Water molecules dissociate (break apart) to produce hydrogen ions (H+) and hydroxide ions (OH-)
43
How to determine acidity vs bascity
Determined by number of free H or OH ions
44
Acids
Molecules that dissociate in water to release H
45
Bases
Either take up H or release OH
46
Oxidized
When an atom loses an electron or when a molecule loses a hydrogen atom
47
Reduced
When an atom gains an electron or molecule gains a hydrogen atom
48
pH
- 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
Biological importance of pH regulation
metabolic reactions, molecular structure, and toxicity of molecules depend on pH
50
Neutralization
- When an equally strong acid & base react - produces water & salt **Ex. HCl + NaOH --> NaCl + H2O**
51
Buffers
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
Buffering blood with hydroxide ions
Water is formed Ex. **OH + H2CO3 --> HCO3 + H2O
53
If a buffer is added to an acidic solution, the pH will ______
Increase
54
If a buffer is added to a basic solution, the pH will ________
Decrease

Biology 12 (14 decks)

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