Nature of molecules, Chapter 2 Flashcards

1
Q

Anatomic number

A

Determine by the number of protons in the nucleus

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2
Q

Anatomic Mass

A
  • Sum of protons and neutrons
  • measured in Daltons 6.02x1023 daltons/1 gram
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3
Q

Cation

A

Positive charge

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4
Q

Anion

A

Negative charge

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5
Q

Isotopes

A
  • Atoms of a single element with a different number of neutrons
  • Named based on their atomic mass
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6
Q

Radioactive Isotope

A
  • unstable meaning their nucleus has a tendency to break apart= Radioactive decay
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7
Q

Half-life

A
  • the time it takes the atoms to decay
  • half of whatever isotopes has decay
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8
Q

Carbon 14

A
  • Use for living tissue bond
  • Carbon isotopes exist natural in known ratios
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9
Q

Bohr Model

A

Way to view anatomic structure, with electrons in discrete orbitals

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10
Q

Orbitals

A

Around a nucleus where electrons are most like

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11
Q

Oxidation

A

loss of electrons

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12
Q

Reduction

A

Gain of electrons

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13
Q

Rule of 8

A

Atoms establish completely full of outer energy levels (8 electrons)

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14
Q

Elements found in the 96.3% weight of your body

A

Carbon, hydrogen, Oxygen, Nitrogen

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15
Q

Ionic Bond

A
  • Attraction of opposite charges, strong
  • Form crystals
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16
Q

Covalent bonds

A

Sharing Electrons pairs, very strong

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17
Q

Hydrogen bonds

A

Sharing of hydrogen atom- has 1 electron

18
Q

Hydrophobic Interaction

A

Forcing of the hydrophobic portion of molecules together in the presence of polar substances, weak

19
Q
  • Double convents bonds
  • Triple covalent bonds
A
  • Share 2 pairs of electrons
  • Strongest covalent bonds
20
Q

Polarity- Nonpolar

A
  • Bonds between identical atoms
  • The affinity for electrons is the same and electrons are shared equally
21
Q

Polar bonds

A
  • Charge is not uniform
22
Q

Chemical reactions

A

formation of making and breaking chemical bonds

23
Q

Reactions

A

Molecules before a reaction starts

24
Q

Products

A

The molecule resulting from a chemical reaction

25
Chemical reactions impacted by?
1) Temperature 2) Concentration of reactants and products 3) Catalysts- substances
26
Water molecules is a?
Polar covalent bond
27
Most important chemical property of water is ?
Hydrogen bonds
28
Cohesion
- Polarity of water allows water molecules to be attracted to one another - Responsible for being a liquid (not gas)
29
adhesion
Water adheres to any substance with which it can form hydrogen bonds
30
Capillary action
water is attracted to polar molecules- this is responsible for capillary action
31
Emergent properties
- Water has a high specific heat - water has a high heat of vaporization - Solid water is less dense than liquid water - Water is good solvent - Water organizes non polar molecules
32
Hydratation shell
Prevents them from associating with other crystal lattice
33
Hydrophobic exclusion
Nonpolar molecules aggregate in water
34
Nonpolar molecules are?
Hydrophobic- not form H-bonds with water
35
Spontaneous ion formation
ionization
36
pH measures?
Concentration
37
Substance that disassociates in water to increase the H+ concentration?
Acid
38
Any substance that combines with H+ when dissolved in water(lowering H+ concentration
Base
39
- Resist changes in pH
Buffer
40
In human blood is an acid-base pair consisting of carbonic acid (acid) and bicarbonate (base)
The key buffer