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BIOS0001 chemistry of life > chemistry exam > Flashcards

chemistry exam Flashcards

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1
Q

What is matter

A

Matter is anything that takes up space and has weight. All matter has volume and weight.

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2
Q

what are the propaties of matter, volume and wieght

A
  • Matter: Occupies space, has weight
  • Volume: Space occupied by matter
  • Weight: Measure of gravitational force acting on matter
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3
Q

what is solid state

A

Particles tightly packed, fixed position

  • Defined shape and size
  • Prevents easy movement through
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4
Q

what is liquid state

A
  • Particles have more space between them
  • Can move past each other
  • No defined shape, but defined volume
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5
Q

what is gas state

A
  • Particles widely spaced
  • No defined shape or volume
  • Allows easy movement through
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6
Q

define the term atom

A

he smallest constituent unit of ordinary matter that constitutes a chemical element

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7
Q

define the term ‘Molecule’

A

particle made up of two or more atoms that are chemically bonded together

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8
Q

define the term ‘Element’

A

a species of atom having the same number of protons in their atomic nuclei

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9
Q

definition of force

A

Force: Any interaction that changes motion of object, such as Causes acceleration in objects with mass

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10
Q

what are the Effects of Force

A

Changes velocity of objects

Causes acceleration

Can be observed as push or pull

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11
Q

what are the characteristics of force

A

Magnitude: Measure of strength

Direction: Indicates where force is applied

Vector quantity: Combines magnitude and direction

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12
Q

where can force be applied

A

to push or pull an object
to change the motion of an object
to cause an object to accelerate

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13
Q

what are the four fundamental forces and does each force do

A

*Gravity –a force that a planet or other body draws objects towards its centre

*Strong force – a force that binds neutrons and protons together to form atomic nuclei

*Weak force – mechanism of interaction between subatomic particles, which is responsible for radioactive decay of atoms

*Electromagnetic force – a force that is attractive or repulsive between two electrically charged objects

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14
Q

what is an atom made up of and what characteristics does each component have

A

proton - Define element, change in number alters element, Heavy, positively charged, Part of nucleus

neutrons - insulate protons, prevent repulsion Neutral, same size as proton part of nucleus, don’t alter atom’s properties

electrons - Bind atoms to form molecules Responsible for chemical reactions, Negatively charged, negligible mass compared to protons/neutrons

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15
Q

What is the mass number?

A
  • Total number of protons and neutrons
  • Represents atom’s mass
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16
Q

What is atomic number?

A
  • Number of protons
  • Unique to each element (what makes the element the element)
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17
Q

What is relative atomic mass?

A
  • Weighted average of isotopic masses. (weighted means the percentage of how prevenance the isotope is in the atmosphere.)
  • Influenced by abundance of isotopes
  • Not always a whole number

E.g. 35Cl and 37Cl isotopes

  • 75% 35Cl, 25% 37Cl in average sample
  • Relative atomic mass of chlorine: 35.45
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18
Q

What are isotopes and example?

A
  • Same number of protons, different number of neutrons, the number of electrons stays the same as the protons
  • Named after element and mass number E.g. carbon 12 has 6 protons and 6 neutrons and carbon 13 has 6 protons and 7 neutrons
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19
Q

What is an ion

A

An ion is where an atom is carrying a charge either positive or negative

  • Anions: Negatively charged, gained electrons
  • Cations: Positively charged, lost electrons
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20
Q

What is radioactive decay?

A
  • Random process from unstable atoms
  • Releases particles and/or energy
  • Predictable by probability in large groups
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21
Q

Types of Radioactive Decay

A
  • Alpha: Helium nucleus, large and slow
  • Beta: High-speed electron/positron, smaller and faster
  • Gamma: High-energy electromagnetic radiation, difficult to stop
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22
Q

What is ionizing radiation

A
  • Electromagnetic radiation or energetic particles
  • Sufficient energy to strip electrons from atoms
  • Examples: X-rays, gamma rays
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23
Q

Types of spectra

A
  • Continuous Spectrum: Uninterrupted range of wavelengths
  • Absorption Spectrum: Produced when atoms absorb energy
  • Emission Spectrum: Produced when atoms release energy, contains colored lines
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24
Q

what is atomic spectra

A

atoms release energy as light. This can look like a coloured line with black line between the colours or the other way around. The colours can look different depending on which element is emitting light.

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25
Q

What is Gas Chromatography-Mass Spectrometry (GCMS)

A
  • Technique to separate and analyze compounds
  • Identifies compounds based on mass-to-charge ratio
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26
Q

what is Fourier-Transform Infrared Spectroscopy (FTIR)

A
  • Obtains infrared spectrum of absorption or emission
  • Used for solids, liquids, or gases
  • Identifies compounds based on infrared absorption patterns
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27
Q

What is Nuclear Magnetic Resonance (NMR)

A
  • Observes nuclei in strong magnetic field
  • distubred by weak oscillating magnetic field
  • Determines molecular structure and composition
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28
Q

What are the Energy Levels of Electrons

A

Back of flashcard:

  • Orbits represent electron energy
  • Ground state: Lowest energy level, closet to the nucleus
  • Excited states: Higher energy levels, the further away they go form the nucleus the more excited the electrons are.
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29
Q

What is the Law of Conservation of Mass?

A
  • Atoms neither created nor destroyed in chemical reaction
  • Atoms rearrange to form different compounds
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30
Q

what can be been as the electrons move between the states

A
  • Light emitted: Electron drops to lower state
  • Light absorbed: Electron moves to higher state
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31
Q

what is the law of definite proportions

A
  • Chemical compound has fixed ratio of elements by mass
  • Ratio consistent regardless of source or method
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32
Q

what is the mole

A

Avogadro’s number: 6.02x10^23 carbon atoms equals to 1 mole.

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33
Q

How is the periodic table organized

A
  • Groups: Vertical columns
  • Periods: Horizontal rows
  • Period indicates number of electron shells
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34
Q

how do the electron shells correlate with the periodic table.

A
  • Dictated by period number
  • Number of electrons = Atomic number
  • Also known as principal quantum number
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35
Q

What is valency

A
  • Valence shell: Outermost electron shell
  • Determines atom’s reactivity by how many
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36
Q

what is the octet rule

A
  • Elements tend to bond to achieve 8 electrons in valence shell
  • Rule of thumb for chemical bonding
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37
Q

What is the principal quantum number (n)

A

the shell number if the shell is number 1 then the principal quantum is also 1

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38
Q

What is the capacity if the subshells and what are there names

A

1st subshell: s, holds up to 2 electrons

  • 2nd subshell: p, holds up to 6 electrons
  • 3rd subshell: d, holds up to 10 electrons
  • 4th subshell: f, holds up to 14 electrons
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38
Q

what is the Electron Capacity of Shells

A
  • 1st shell: Holds up to 2 electrons
  • 2nd shell: Holds up to 8 electrons
  • 3rd shell: Holds up to 18 electrons
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39
Q

What are orbitals

A

electrons are not laided out in neat circles as depicted in textbooks

Electrons occupy orbitals within subshells

  • Different configurations within same subshell
  • Governed by Pauli Exclusion Principle
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40
Q

Reactivity within the elements

A
  • Elements on left of periodic table tend to lose electrons
  • Group 1 elements have 1 electron in valence shell
  • Atoms with more shells are more reactive due to weaker nucleus-electron attraction
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41
Q

What polarity of water

A

water molecules are polar due to unequal sharing of electron.

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42
Q

Define a Solute

A

A solute is a substance being dissolved

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43
Q

Define a solvent

A

The solvent is the medium which dissolves the solute

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44
Q

Define solution

A

A solution is defined as mixture consisting of a solute dissolved into the solvent. Can’t be filtered out.

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45
Q

What is the composition of water

A

2 hydrogen atoms and 1 oxygen atom. Joined together by hydrogen bond

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46
Q

what is an aqueous solution

A

a solution where the solvent is water. In a equation this is written as (aq)

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47
Q

What are the Distinctive properties of water

A
  • High boiling point (100°C)
  • High surface tension
  • Specific heat
  • Heat of evaporation
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48
Q

What is electrolysis and why does

A

Electrical current is used to break down compounds into elements. Ions move towards opposite charge electrodes

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49
Q

what is the ion movement in electrolysis

A

Positive ions (cations) move towards (-)

Negative ions (anions) move towards move anode (+)

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50
Q

What is self ionisation of water

A

one water molecules donates a proton to another water molecule

rapid processes

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51
Q

What is the application of self ionisation

A

equilibrium process applicable to diluted aqueous solutions. - Can determine [H+] if [OH-] is known

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52
Q

what is acid base equilibrium

A

The transfer of protons in both forward and reverse reactions.

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53
Q

what is a forward reaction

A

Bronsted-lowry acid donates proton
bronsted-lowry base accepts proton

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54
Q

what is a reverse reaction

A

acid and base switch roles and in doing so become conjugate bases of each other, so an acid can accept an proton and a base can donate a proton.

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55
Q

What does it mean when a substance is amphoteric

A

A substance that can donated and accept electrons. Therefore it can be a acid or base

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56
Q

what is Arrhenius theory

A

Acids dissociate in water to produce hydrogen ions. (H+)
Bases ionize in water to produce hydroxide ions

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57
Q

what are advantages of Arrhenius theory

A

describes properties of acids and bases
indicates the strength of acids and bases
confirms concepts of neutralization hydrolysis

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58
Q

what is a conjugate base

A

A conjugate base is an ex acid that has lost it positively charged proton.

A conjugate base can return back to an acid if it accepts a proton

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59
Q

What is a conjugate acid

A

A conjugate acid is a ex base that has accepted a proton

a conjugate acid can return back to an base if donates it proton.

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60
Q

what is the disadvantage of the Arrhenius theory

A

only describes acid-base chemistry in aqueous solutions

61
Q

what are the role of acids and bases in Bronsted-lowry and Arrhenius theory

A

Acid donates protons
base accepts protons

62
Q

How to identify acids and bases in Bronsted-Lowry

A

count the protons to determine acid or bases

63
Q

what is the relationship between acid strength

A

stronger the Bronsted-Lowry acid, the weaker the conjugate base

stronger Bronsted-Lowry base, weaker acid

64
Q

what is a monoprotic acid

A

transfers one proton per molecule in an acid-base reaction

65
Q

What is a diprotic acid

A

transfers two proton per molecule in acid-base reaction

66
Q

what is a triprotic acid

A

transfers three proton in acid-base reaction

67
Q

what is a polyprotic acid

A

Transfers two or more protons per mole in acid-base reaction.

68
Q

What dissociation constant of water

A

Neutral solution H+ = OH-

69
Q

What is the definition of pH

A

pH stands for potential of hydrogen. Measures the concentration of hydrogen ions in a substance.

70
Q

what doe the pH scale identify

A

pH scale identifies acidity or basicity of aqueous solutions

71
Q

what are the proprieties of an acidic solution on a pH scale

A

Lower on pH scale
higher concentration of hydrogen ions (H+)

72
Q

what are the proprieties of an alkaine soltuion on the pH scale

A

higher on the pH scale
lower concentration of hydrogen ions (H+)

73
Q

what is the difference between pH and pOH

A

pH measures hydrogen concentration

pOH measures hydroxide concentration

74
Q

what is a buffer

A

buffers have a working pH range and capacity. Meaning buffers can resit change when acids or bases are added and can neutralize small amounts of acids and base.

buffers maintains constant pH.

75
Q

what are the components of buffers

A

consists of either a weak acid and a conjugate base or weak base and a conjugate acid

76
Q

examples of buffers

A

Acetic acid acid (CH3COOH) and sodium acetate (CH3COONa)

Ammonia (NH3) and ammonium hydroxide (NH4OH)

77
Q

what are chemical reactions

A

Process where molecular structure changes
Useful in cooking, combustion, photosynthesis, respiration

78
Q

what is flame photometry used for

A

used for identification of metal ions

79
Q

how do bond breaks and form in compounds

A

bonds between the reactants most be broken and new bonds formed in the compounds

80
Q

what is a compound

A

a substance of two or more elements in a fixed ratio and are formed by a chemical bond

81
Q

what is a mixture

A

A Physical combination of substances that are Not chemically joined.

82
Q

what are reactants

A

the substances at a beginning of a chemical reaction.

83
Q

what are the products

A

substances at produced by a reaction

84
Q

what are the signs of a chemical reaction

A

Physical change
Colour change
Temperature change
Gas release
Formation of a precipitate

85
Q

Examples of Reactants and Products

A
  • Methane + Oxygen → Carbon dioxide + Water
  • Iron + Sulfuric acid → Iron sulfate + Hydrogen gas
  • Sodium hydroxide + Hydrochloric acid → Sodium chloride + Water
  • Nitric acid + Sodium carbonate → Sodium nitrate + Carbon dioxide + Water
86
Q

what is a synthesis reaction

A

Two or more elements/compounds form complex product

87
Q

what is a decompostion reaction

A

One reactant breaks into two or more products

88
Q

what is a displacement reaction

A

More reactive element displaces less reactive one in compound

89
Q

what is a double displacement reaction

A

Cations and anions of two compounds exchange

90
Q

what is a combustion reaction

A

Fuel combines with oxygen

91
Q

what is a incomplete combustion reaction

A

Insufficient oxygen leads to formation of CO, carbon, and water

92
Q

what is a redox reactions

A

where both Oxidation (Addition of oxygen) and Reduction (Removal of oxygen) take place

93
Q

what is a endothermic reactions

A

Absorb energy from surroundings,
Products and surroundings become cold
ENDO - internal energy comes in

94
Q

what is a exothermic reactions

A

Release energy to surroundings
Products have less energy than reactants
EXIT - energy exits

95
Q

what is ∆H in Endothermic Reactions

A

∆H: Amount of energy input
∆H positive: Products utilize energy of reactants

96
Q

what is ∆H in Exothermic Reactions

A

∆H: Amount of energy released
∆H negative: Products have less energy than reactants

97
Q

what are reversible reactions

A

Conversion of reactants to products and vice versa occur simultaneously

e.g. A + B ↔ C + D
C + D ↔ A + B

98
Q

what is the definition of equilibrium

A

Forward and backward reactions occur at same rate

99
Q

what is Le Chatelier’s Principle

A

Le Châtelier’s principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish an equilibrium.

100
Q

what is the Haber process in equilibrium

A

this is the reaction - N2 + 3H2 ⇌ 2NH3

haber process converts nitrogen and hydrogen to ammonia

101
Q

how does concentration affect equilibrium

A

Removing products shifts equilibrium towards making more reactants

102
Q

how does temperature affect equilibrium

A

higher Temp favors endothermic reaction, lower favors exothermic

103
Q

How does pressure affect equilibrium

A
  • higher Pressure shifts to fewer moles, lower to more moles
104
Q

what is equilibrium expression

A

K indicates reactant and product concentrations at equilibrium

105
Q

how is K interpreted

A

K > 1: More products
K < 1: More reactants

When K is between 0.0001 and 1000 means that there is a significant mix of reactants and products

106
Q

what is the definition of energy

A

ability to do work

follows laws of conversation of energy

107
Q

what is the law of conversation of energy

A

energy can’t be created or destroyed, only converted

108
Q

What is the SI unit of energy

A

Joule (J)

109
Q

heat and work are both examples of energy what are there properties

A

heat - Transfer from hot to cold object and the Motion of atoms and molecules

work - is energy transferred by the movement of objects.

110
Q

Definition of enthalpy

A

energy change at constant pressure

111
Q

what is the symbol of enthalpy

A

H

112
Q

what is enthalpy change

A

ΔH = Heat lost or gained by system under constant pressure

113
Q

is enthalpy a thermodynamic property

A

yes as it is a property of system. (a propetry of a system means something we can measure such as temperature and volume)

114
Q

what is the formula of enthalpy

A

Reflects capacity for non-mechanical work and heat release

115
Q

How is enthalpy measured

A

enthalpy is measured by the change in enthalpy because total enthalpy cannot be directly measured

116
Q

what is Hess’ law

A

Hess’ law states that the change in energy is dependent only on the beginning and end states.

117
Q

what is entropy

A

measurement of disorder or molecular randomness (S)

118
Q

is entropy a thermodynamic property

A

yes as it is a property of system like enthalpy

119
Q

what is the tendency of entropy

A

the natural tendency for entropy (S) to increase

120
Q

entropy in chemical reactions

A

More bond breaking = More entropy
as the States change, more moles of products than reactants

121
Q

what can entropy measure in a system

A

energy distribution

122
Q

what is the 2nd law of thermodynamic

A

2nd Law of Thermodynamics

Entropy of universe increases in spontaneous process
Remains unchanged in equilibrium process

123
Q

what is Gibbs Free Energy

A

Amount of energy free to do useful work in a system

124
Q

how to measure Gibbs free energy

A

ΔG = ΔH - TΔS
ΔH: Enthalpy
ΔS: Entropy
T: Absolute temperature

125
Q

Where is Gibbs free energy in biology

A

Living cells constantly require energy
Open system, materials in/out, recycling of products
cells go Against equilibrium and entropy

126
Q

what is a spontaneous reaction

A

Exergonic: ΔG < 0
Gibbs free energy change is negative
Reaction occurs spontaneously

127
Q

what is a nonspontaneous reaction

A

Endergonic: ΔG > 0
Gibbs free energy change is positive
Energy absorbed, reaction nonspontaneous

128
Q

what is the Triple Point in a phase diagram

A

Temperature and pressure allow solid, liquid, and gas phases simultaneously

129
Q

what is Critical Point in a phase diagram

A

Temperature and pressure merge gas and liquid phases

130
Q

what is the sublimation

A

transition from solid to gaseous state

131
Q

Sublimation Process

A

Endothermic and Occurs below substance’s triple point

132
Q

what is the structure of carbohydrates

A

Basic monomer: Saccharide (sugar) Single monomer: Monosaccharide
Two monomers: Disaccharide (bonded by glycosidic bonds)
Large chain of monomers: Polysaccharide

133
Q

what are monosaccharides

A

Sweet taste and soluble
General formula: (CH2O)n where ‘n’ is a number between 1 and 7 (commonly 5 or 6)
Examples: Glucose, galactose, fructose

134
Q

what is glucose

A

Hexose sugar (6 carbon atoms)
Formula: C6H12O6
Two isomers: Alpha glucose and beta glucose

135
Q

when do condensation reactions happen

A

Condensation reactions happens when monosaccharides combined in pairs to form disaccharides with glycosidic bonds.

136
Q

what is hydrolysis

A

Process of breaking down polymers and disaccharides into monomers
Involves breaking bonds with water molecules

137
Q

what is starch

A

Polysaccharide made of chains of alpha glucose
Functions as a storage molecule in plants and a main energy source in human diet
Insoluble and compact, making it ideal for storage and transportation Can be hydrolysed into alpha glucose for use in respiration

138
Q

what is glycogen

A

Made of alpha glucose with more branches than starch
- Functions as carbohydrate storage in animals
- Stored as granules in muscles and liver cells
- Insoluble, compact, and easily hydrolyzed for quick energy release

139
Q

what is cellulose

A

Made of beta glucose units
Chains run parallel and are connected by hydrogen bonds
Provides rigidity and structure to plant cell walls
Prevents cells from bursting open and supports turgidity for photosynthesis

140
Q

what are lipids

A

Diverse group soluble in organic solvents
Non-polar due to C-H and C-C bonds
Contains carbon, hydrogen, and oxygen
Examples: triglycerides, waxes, steroids, cholesterol

141
Q

what is the role of lipids

A

Mainly an energy store
Stores over twice the energy of carbs (~38 kJ/g)
Stored in adipose tissue for insulation and organ protection
Important for plasma membrane structure and repair

142
Q

what are triglycerides

A

Comprised of glycerol (C3H8O3) and three fatty acids
Glycerol has three hydroxyl groups (OH)
Function: Energy storage, most common fat in the human body
Formation: Ester bond between glycerol’s OH and fatty acids’ COOH through condensation
Can have same or different fatty acids

143
Q

Saturated vs. Unsaturated Fatty Acids

A

Saturated fatty acids: Single bond carbon atoms, straight molecules
Unsaturated fatty acids: Contains double bonds, creating kinks
Monounsaturated: One double bond
Polyunsaturated: More than one double bond
Cis-/trans-: Refers to the arrangement of atoms or groups around double bonds

144
Q

what are phospholipids

A

Glycerol subunit with two fatty acid tails and a phosphate group
Main components of cell membranes
Structure includes hydrophilic (water-loving) head and hydrophobic (water-hating) tail
Hydrophilic head interacts with water but not fat
Hydrophobic tail mixes with fat but not water

145
Q

what is DNA structure

A

DNA stands for Deoxyribonucleic acid
Two strands winding around each other like a ladder
Sides of the ladder made of pentose sugar and phosphate groups arranged alternately
Rungs of the ladder made of nitrogenous bases: adenine (A), Thymine (T), guanine (G), and cytosine (C)
Adenine and guanine are purines, while thymine and cytosine are pyrimidines

146
Q

what is RNA Structure

A

RNA stands for Ribonucleic acid
Polymer made up of nucleotides
Ribose sugar attached to a phosphate group and a nucleotide
Contains adenine (A), cytosine (C), guanine (G), and uracil (U)
Uracil replaces thymine in RNA

147
Q

what are vitamins

A

Essential molecules for proper cell function
Obtained through diet because the body can’t produce most vitamins
Previously thought to be amino acids, but only some vitamins contain amino groups

148
Q

what is hydroxylation

A

a chemical process that introduces a hydroxyl group into an organic compound.

149
Q

what is vitamin D

A

Steroid hormone
Two types: Ergocalciferol (D2) from diet, Colecalciferol (D3) made from cholesterol
Synthesized in skin with UVB radiation from sunlight

150
Q

Vitamin D activation

A

Front of flashcard:
Vitamin D Activation

Colecalciferol (D3) and ergocalciferol (D2) converted to calcifediol (25(OH)D) in liver
Calcifediol activated in kidneys to alfacalcidol and calcitriol (1,25(OH)2D)
Calcitriol deactivated in kidneys to 1a,24,25-trihydroxycolecalciferol
Excretion within hours to days
Calcitriol is active form; excess associated with abdominal pain, UTIs, weakness, nausea

BIOS0001 chemistry of life (1 decks)

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