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A&P1 > Week 4: Cellular Biology > Flashcards

Week 4: Cellular Biology Flashcards

1
Q

Element

A

simplest form of matter to have unique chemical properties

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2
Q

Atomic Number

A

number of protons in its nucleus

Elements arranged by atomic number

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3
Q

Electrolytes

A

mineral salts needed for nerve and muscle function

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4
Q

Minerals

A
  • inorganic elements extracted from soil by plants and passed up food chain to humans; Example: Ca, P, Cl, Mg,K, etc.
  • about 4% of body weight
  • important for body structure ie. Ca crystals in teeth, bones, etc.
  • important for body structure
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5
Q

Nucleus

A

Center of atom; made up of protons & neutrons

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6
Q

Protons

A

Single + charge; mass = 1 amu

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7
Q

Neutrons

A

No charge; mass= 1 amu

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8
Q

Atomic Mass

A

Sum of protons & neutrons; accounts for the fact that an element is a mixture of isotopes & is close to the mass of the most abundant isotope.

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9
Q

Eletrons

A

Single - charge; very little mass

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10
Q

Valence Electrons

A

orbit the most outermost shell & determine chemical bonding properties of an atom

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11
Q

Isotopes

A

varieties of an element that differ only in the number of neutrons; isotopes of an element are chemically similar because they have the same number of valence electrons

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12
Q

Matter

A

anything that occupies space and has mass

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13
Q

Energy

A

the ability to do work

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14
Q

96% of body is made up of these elements

A

4: carbon, oxygen, hydrogen, and nitrogen

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15
Q

Atoms

A

Building blocks of elements

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16
Q

Radioisotope

A
  • heavy isotope
  • tends to be unstable
  • Decomposes to more stable isotope
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17
Q

Radioactivity

A

process of spontaneous atomic decay

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18
Q

Molecule

A

two or more like atoms combined chemically

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19
Q

Compound

A

two or more different atoms combined chemically

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20
Q

Atoms formed with

A

Chemical Bonds

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21
Q

How do atoms dissociate?

A

Breaking of chemical bonds

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22
Q

Electron Shells

A

-electrons occupy energy levels
-Electrons closest to the nucleus are most strongly attracted
-Each shell has distinct properties:
The number of electrons has an upper limit
Shells closest to the nucleus fill first

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23
Q

Which electrons are involved in bonding?

A
  • Bonding involves interactions between electrons in the outer shell (valence shell)
  • Full valence shells do not form bonds
24
Q

Inert Elements

A

Atoms are stable (inert) when the outermost shell is complete

25
Q

Electron Shell Capacity

A

Shell 1 can hold a maximum of 2 electrons
Shell 2 can hold a maximum of 8 electrons
Shell 3 can hold a maximum of 18 electrons

26
Q

Rule of Eights

A

Atoms are considered stable when their outermost orbital has 8 electrons
The exception to this rule of eights is Shell 1, which can only hold 2 electrons

27
Q

How atoms reach stable state ?

A

Atoms will gain, lose, or share electrons to complete their outermost orbitals and reach a stable state

28
Q

Chemically inert element exampls

A

Hydrogen: 2 electrons; Neon= 10 electrons (2 in the inner shell, 8 in the second electron shell)

29
Q

Reactive Elements

A

-Valence Shells are not full and are unstable
Tend to gain, lose, or share electrons
Allow for bond formation, which produces stable valence

30
Q

Types of bonds

A

1.ionic
2. covalent
3.hydrogen
4.

31
Q

Ionic Bonds

A

Form when electrons are completely transferred from one atom to another

32
Q

Ions

A

Either donate or accept electrons

33
Q

Anions

A

Negative Charge

34
Q

Cations

A

Positive Charge

35
Q

Covalent Bonds

A
  • Atoms become stable through shared electrons
  • Single covalent bonds share one pair of electrons
  • Double covalent bonds share two pairs of electrons
36
Q

Single Covalent Bond Example

A

H2, CH4

37
Q

Double Covalent Bond Example

A

O2

38
Q

Polarity

A

Covalently bonded molecules

  • Some are non-polar: Electrically neutral as a molecule
  • Some are polar: Have a positive and negative side
39
Q

Non-polar bond examples

A

CO2

40
Q

Polar bond examples

A

H20

41
Q

Hydrogen Bonds

A
  • Weak chemical bonds
  • Hydrogen is attracted to the negative portion of polar molecule
  • Provides attraction between molecules
42
Q

Synthesis Reaction

A

A+B => AB

  • Atoms or molecules combine
  • Energy is absorbed for bond formation
43
Q

Decomposition reaction

A

AB->A + B

  • Molecule is broken down
  • Chemical energy is released
44
Q

Synthesis Reaction example

A

Amino acids -> protein molecule

45
Q

Decomposition Reaction

A

Glycogen-> glucose units

46
Q

Exchange Reaction

A

AB + C–> AC + B

  • Involves both synthesis and decomposition reactions
  • Switch is made between molecule parts and different molecules are made
47
Q

Exchange Reaction Example

A

Glucose + ATP –> Glucose Phosphate + ADP

48
Q

Organic Compounds

A

Contain carbon
Most are covalently bonded
Example: C6H12O6 (glucose)

49
Q

Inorganic compounds

A

Lack carbon
Tend to be simpler compounds
Example: H2O (water)

50
Q

Water Vital Properties

A
  • High heat capacity
  • Polarity/solvent properties
  • Chemical reactivity
  • Cushioning

**Most abundant inorganic compound

51
Q

Salts

A
  • Easily dissociate into ions in the presence of water
  • Vital to many body functions
  • Include electrolytes which conduct electrical currents
52
Q

Acids

A
  • Release hydrogen ions (H+)

- Are proton donors

53
Q

Bases

A
  • Release hydroxyl ions (OH–)

- Are proton acceptors

54
Q

Neutralization reaction

A

Acids and bases react to form water and a salt

55
Q

pH

A

Measures relative concentration of hydrogen ions
pH 7 = neutral
pH below 7 = acidic
pH above 7 = basic

56
Q

Buffers

A

chemicals that can regulate pH change

A&P1 (15 decks)

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