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B.Sc in Biomedical Engineering > CHM104 - Chemistry for Life Sciences > Flashcards

CHM104 - Chemistry for Life Sciences Flashcards

1
Q

What is Chemistry?

A

Chemistry is a field of science dealing with how matter & energy interact with each other.

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2
Q

What are the phases of matter?

A
  • Solid phase/state
  • Liquid phase/state
  • Gaseous phase/state
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3
Q

What is the key characteristic of a Liquid phase?

A

It has an indefinite shape but fixed volume.

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4
Q

What is the key characteristic of a Solid-phase?

A

It has a fixed shape & volume.

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5
Q

What is the key characteristic of the Gaseous phase?

A

It has no fixed shape & volume.

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6
Q

What are the types of mixtures?

A
  • Homogenous mixtures & non-homogenous mixtures
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7
Q

What are Homogenous mixtures/Solutions?

A

Homogenous mixtures or solutions are mixtures which are uniformly mixed. Example: Sea water.

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8
Q

What are Heterogenous mixtures?

A

These are the mixtures which are non-uniformly mixed. Example most rocks like Granite (Having Feldspar, quartz & mica).

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9
Q

What are the methods of separation of mixtures?

A
  • Distillation
  • Filtration
  • Mass Spectrometry
  • Chromatography
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10
Q

What is Mass spectrometry?

A

It is a method of separation of mixtures by the atomic mass.

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11
Q

Quantity, what is it?

A

It means you can assess the measurable value of a measurement.

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12
Q

What is the Metric system based on?

A

It’s a system based on decimal points.

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13
Q

What is Acetone (CH3COCH3) used for?

A

Acetone is an organic compound used to dissolve other solvents.

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14
Q

Instruments to measure Length?

A

The Metre Rule is used to measure the Length & the standard unit is in Metres (m).

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15
Q

Conversion of Millilitres to Cm3, please?

A

1mL = 1cm3

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16
Q

What are the instruments to measure Volume?

A
  • Pipette
  • Burette
  • Graduated cylinder
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17
Q

What is Mass?

A

Is the amount of matter in an object

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18
Q

What is weight?

A

It’s the gravitational force acting on an object

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19
Q

What do we use to Reset the weight of the weighing container on a weighing balance?

A

The Tare button.

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20
Q

What is the mechanism of Heat flow?

A

Heat flow is such that it flows from an object with high temperature to an object with low temperature.

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21
Q

Formulae for conversion of Temperature from degrees centigrade to Fahrenheit:

A

Tf = (1.8)Tc + 32

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22
Q

Formulae for conversion of Temperature from degrees Fahrenheit to degrees centigrade:

A

(Tf - 32) / 1.8 = Tc

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23
Q

Your decimal points in your answers should..?:

A

Match the decimals you were given in your question. (For addition or subtraction problem)

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24
Q

What does Intravenously means?

A

The drug delivery method in the body through the veins

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25
Q

Significant figures & calculations:

A

Take the value with less significant figures from the data given & assign the same to your final answer. Especially in division or multiplication.

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26
Q

What is Matter?

A

Matter is anything that occupies space and it has mass.

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27
Q

What is an alloy?

A

An alloy is a solid mixture of two or more substances making a same composition throughout.

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28
Q

What is the difference between an element & a compound?

A

An element is a pure substance which is made up of one kind of atom,
WHILE:
A Compound is a pure substance which is made of of more than one kind of atom.

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29
Q

What is a solution?

A

A solution is a mixture with the same composition throughout.

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30
Q

How many elements are there so far? And which ones occur naturally?

A

There are 118 known elements so far, of which 91 occur naturally.

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31
Q

Mercury in Latin please (Teaser):

A

Hg (Hydrargyrum)

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32
Q

Key distinguisher between Compounds & Mixtures:

A

Compounds have fixed compositions in the same percentages by mass.
While Mixtures have varying compositions.

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33
Q

What are the tools to measure volume?

A

Measuring Cylinder, Pipette & Burette.

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34
Q

What are pure substances?

A

They are either elements or compounds

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35
Q

What’s an element?

A

A type of matter which can’t be broken down into two or more pure substances.

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36
Q

What’s a chemical symbol?

A

A chemical symbol is the chemical representation of a chemical substance in form of letters. Mostly, 1 or 2 letters.

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37
Q

What’s a compound?

A

A pure substance is made up of more than one element. e.g Water is a compound made of Hydrogen & Oxygen.

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38
Q

What is the comment on Compounds & their compositions?

A

Compounds have a fixed composition (Same elements in the same percentage by mass)

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39
Q

Are elements & compounds’ characteristics the same?

A

No. Usually, the elements & compounds characteristics are different. E.g Na, Cl & NaCl

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40
Q

What are some ways to split compounds?

A
  • Electrolysis
  • Heating
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41
Q

What is a mixture?

A

A mixture comprises of 2 or more substances combined in a way that the substance retain their chemical identity.

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42
Q

What comprises a solution?

A

A solution comprises of a SOLVENT & SOLUTE. Solvent is usually in the largest amount.

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43
Q

In a Solution, what can Solute be?

A

It can be a liquid, solid or gas.

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44
Q

What is an example of a Solid solution?

A

Brass - It’s made up of Copper & Zinc.

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45
Q

What is distillation?

A

Is a method of separating homogenous solid-liquid mixtures by vaporization & condensation of the liquid, leaving behind the residue solute.

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46
Q

What is filtration?

A

A method to separate heterogeneous mixtures by using a barrier with fine pores like filter paper.

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47
Q

What is chromatography?

A

It’s a method of separation of a mixture by the use of solubility or extent of adsorption on a solid surface.

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48
Q

What is a Metric system?

A

Is a measurement system where the units are measured in the powers of ten.

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49
Q

What is temperature?

A

Temperature is a factor that determines the direction of heat flow.

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50
Q

What are Celsius?

A

A unit of temperature with a 100 degrees range based on the the freezing & boiling points of water.

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51
Q

What causes the degree of uncertainty in measurements?

A

The Nature of the instrument & The skill of the operator.

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52
Q

What is a conversion factor?

A

A ratio, numerically equal to 1 by which a quantity can be converted from one unit to another.

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53
Q

What’s another name for the Conversion factor?

A

Dimensional analysis

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54
Q

What are Bridge conversions?

A

They are conversion ratios allowing you to transfer from the English metric system to the Metric system.

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55
Q

What does pulvarize mean?

A

Making into powder (powderize), by breaking up or making into dust.

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56
Q

What are Intensive properties?

A

They are the properties that Identify a substance. They are independent of the amount.

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57
Q

What are Extensive properties?

A

They are the properties that are dependent on the amount.

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58
Q

What other properties (apart from the intensive & extensive) that we can use to identify chemical substances?

A
  • Chemical properties
  • Physical properties
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59
Q

What are Chemical properties?

A

They are the properties observed as a substance takes part in a chemical reaction. e.g Inertdness of Helium, reactiveness of hydrogen.

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60
Q

What are Physical properties?

A

They are the properties which are observed without even changing the Identity of the chemical substance. e.g: Boiling point & melting point.

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61
Q

What’s the melting point?

A

The temperature at which the substances change from solid to liquid.

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62
Q

What’s the boiling point?

A

The temperature at which the substance changes from liquid to gaseous state.

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63
Q

What is density?

A

Density of a substance is the ratio of mass to volume

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64
Q

How is the volume of irregular solids obtained?

A

By displacement method of a liquid.

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65
Q

How is the MASS of regular solids obtained?

A

By direct weighing.

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66
Q

What is Solubility?

A

is the process by which the Solute dissolves in a solvent.

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67
Q

What type of change is Solubility?

A

A Physical change/

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68
Q

What’s the chemical formula for Sucrose?

A

C12H22O11

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69
Q

What is a Saturated solution?

A

A solution in equilibrium with undissolved solute.

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70
Q

What is an Unsaturated solution?

A

A solution containing less solute than the equilibrium.

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71
Q

What is a Supersaturated solution?

A

A solution containing more solute than the amount allowed at equilibrium.

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72
Q

What can Potassium permanganate be used as?

A

As an antiseptic (Cleaner) to infections

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73
Q

What are cations?

A

These are positively charged ions

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74
Q

What are anions?

A

These are negatively charged ions

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75
Q

Why do things colorate? e.g fruits when left in air etc..

A

Due to oxidation

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76
Q

What can you comment on temperature & oxidation?

A

Lowering temperature decreases the rate of oxidation.

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77
Q

Denote these:
- Atomic number
- Mass number

A

Atomic number = Z
Mass Number = A

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78
Q

What is Atomic number?

A

Atomic number is the number of protons in the nucleus of an atom.

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79
Q

What is Mass number?

A

The mass number is the summation of the number of protons & number of neutrons in a nucleus of an atom.

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80
Q

What are Isotopes?

A

These are atoms with the same number of protons but a different number of neutrons. Example: C-12 & C-14.

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81
Q

What techniques can we use to reduce the rate of Oxidation?

A
  • Refrigeration
  • Placing an item in water
  • Adding vinegar
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82
Q

What is the use of these Chemicals?
- Potassium permanganate
- Antimony
- Glycerol

A

These are their uses respectively:
- Potassium permanganate - as an antiseptic in cleaning infections & wounds.

  • Antinmony - It is used to detect leakage in oil pipes
  • Glycerol - It is used to sweeten drinks & as a food thickener.
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83
Q

What’s the remedy for people who can’t sleep?

A

A glass of lukewarm milk

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84
Q

Which metal can melt at room temperature?

A

Gallium

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85
Q

What is the use of Sodium Bicarbonate (Baking Soda) for everyday home use?

A

To absorb odor.

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86
Q

What are Dalton’s atomic theory principles?

A
  • An element is comprised of tiny particles called atoms
  • Atoms of a given element have the same chemical properties (atoms of diff…visa versa)
  • In a chemical reaction, atoms move from one substance to another, atoms never disappears or changed into an atom of another element
  • Compounds are formed when atoms of 2 or more elements are combined (And the relative numbers of each atoms are constant & definite)
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87
Q

What is an atom?

A

It’s the smallest part of an element that retains the chemical properties of that element.

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88
Q

How did the first discoveries of subatomic particles come by?

A

It were the Electrons which were discovered by passing electricity to gases at low pressure.

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89
Q

What are electrons?

A

They are the negatively charged sub-atomic particles which are found outside the nucleus.

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90
Q

What is the unit charge of an electron?

A

-1

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91
Q

What is the experiment by J.J Thomson that shows that the electrons are negatively charged & are present?

A

Passing a Cathode Ray in a cathode tube toward a Zinc Sulfide screen will deflect the ray to the positive plate showing that the electrons are negatively charged.

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92
Q

About atoms reacting, what LAW did J.J Dalton Atomic theory cover?

A

Law of conservation of mass
Law of Constant composition

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93
Q

State the Law of Constant composition:

A

Compounds always contain the same elements with the same proportions by mass.

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94
Q

About atoms reacting, what LAW did J.J Dalton Atomic theory cover?

A

Law of conservation of mass
Law of Constant Composition

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95
Q

State the Law of conservation of Mass:

A

In a normal reaction, there is no detectable change in mass in an ordinary atom.

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96
Q

State the law of multiple proportions, & where does it apply to?

A

“The masses of one element that combine with a fixed mass of a second element are in a fixed ratio of small numbers”

  • It applies when 2 atoms form more than one compound.
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97
Q

Who proposed the first model that electrons are embedded in a positive charge cloud sphere in an atom?

A

J.J Thomson

98
Q

What are Alfa particles?

A

They are helium atoms without their electrons

99
Q

What’s the nucleus?

A

It;s the small densely positively charged part at the centre of an atom

100
Q

Who made the experiments of the atom in discovering that the nucleus is positively charged?

A

Ernest Rutherford as the alfa particles were deflected by the nucleus of an atom.

101
Q

What’s the charge of a proton?

A

+1, and is equal to that mass of a Hydrogen atom.

102
Q

What’s the Neutron?

A

It’s the uncharged particle of the nucleus of an atom with a mass slightly greater than that of a proton.

103
Q

Why is the mass of an atom concentrated at the nucleus?

A

because the proton & the neutron are there. They are heavier in mass than the electron

104
Q

What is the atomic number (Z)

A

It’s the number of protons in an atom

105
Q

What is the mass number (A)

A

It’s the total number of protons & neutrons in a nucleus of an atom.

106
Q

What’s an Isotope?

A

An atom with the same number of protons but different neutrons. Example: Hydrogen (Light hydrogen = 0 Neutrons, Deuterium = 1 neutron & Tritium = 2 neutrons)

107
Q

What does a nuclear symbol show us?

A

It shows a composition of the nucleus of an atom.

108
Q

Why do we call it the “Relative mass”?

A

because actual atoms are hard to measure by a balance on themselves, so we use a scale in relation to the mass of Carbon-12 atom.

109
Q

What is atomic mass/atomic weight?

A

It’s the AVERAGE mass of an atom measured RELATIVE to that of another element, using the Carbon-12 scale.

110
Q

What is the Carbon-12 scale?

A

An atomic mass scale where the mass of Carbon is assigned 12 amu exactly.

111
Q

How are the relative masses of atoms determined?

A

By using a Mass Spectrometer

112
Q

Why do we have to determine the Isotopic abundances of elements?

A

Because mostly elements don’t just occur as single isotopes, rather more than 1 isotope.

113
Q

What is the Avogadros Number?

A

It’s the number of units in a Mole

114
Q

What does the Avogadros Number represent?

A

It represents the number of atoms in an element whose mass in grams is numerically equal to the element’s atomic mass.

115
Q

What are Periods?

A

They are horizontal rows in the Periodic table

116
Q

What are groups?

A

They are the Vertical columns in the periodic table

117
Q

What are the main group elements?

A

They are the elements of group 1,2 and 13 to 18.

118
Q

What are the Transitional elements?

A

They are the elements which fall between groups 3 to 12. And period 4 to 6.

119
Q

What are post-transitional elements?

A

They are the elements in groups 13 to 15.

120
Q

What are alkali metals?

A

They are the elements in Group 1 of the periodic table.

121
Q

What are alkaline earth metals?

A

They are elements in group 2

122
Q

What are Halogens?

A

They are the elements in Group 17

123
Q

What are Noble gases?

A

They are the elements in Group 18

124
Q

What can you comment on the elements being in the same group?

A

They usually have the same chemical properties.

125
Q

What’s the formal definition of a periodic table?

A

It’s a table showing the arrangement of elements in an increasing atomic number, in such a way that the elements of the same chemical properties fall in the same group.

126
Q

What are metals?

A

Substances with characters of malleability, luster, & high electrical conductivity.

127
Q

What are metalloids?

A

They are elements which have characters of both metals & non-metals.

128
Q

What elements do exist alone mostly?

A

Inert gases

129
Q

What does the combination of elements create?

A

Molecules & ions

130
Q

What are molecules?

A

A combination of atoms combined covalent to form compounds.

131
Q

What forces hold the molecules?

A

Covalent forces

132
Q

What’s a molecular formula?

A

A chemical formula showing the number of atoms in each element, discretely. The number of atoms are written as subscript below each chemical symbol.

133
Q

What’s structural formula?

A

A chemical formula showing structure of bonded atoms in a molecule.

134
Q

What is a condensed structural formula?

A

It’s the chemical formula showing the functional group of that chemical. e.g CH3C00H - Acetic acid

135
Q

What are ions?

A

They are the charged atoms when the atom looses or gains electrons

136
Q

What kind of bond holds the Polyatomic ions?

A

Covalent bonds

137
Q

What’s an ionic compound?

A

A compound formed by both Cations & Anions. e.g NaCl

138
Q

What are ionic bonds?

A

Strong electrostatic forces holding together cations & anions in an ionic bond.

139
Q

Why do Ionic compounds have high melting points?

A

Because the energy required to separate the cations in these ionic bonds is very huge

140
Q

Why can we call NaCl an electrolyte, when we call Sugar a Non-electrolyte?

A

Because once in the water, the Solution of NaCl conducts electricity while that of Sugar doesn’t.

141
Q

What is the principle of Electric Neutrality?

A

It states that in any compound, the total positive charge must equal to the total negative charge

142
Q

Why are noble gases unreactive?

A

Because they are so Stable.

143
Q

Which metals do not follow the noble gases stability structure?

A

The Transitional & post-transitional metals

144
Q

What are the common polyatomic cations?

A

NH4+ (Ammonium) & Hg2+ (Mercury I)

145
Q

What’s the rule for naming monoatomic cations?

A

By taking the name of the metal. And the anion has an -ide suffix.

146
Q

How are the names of the Transition Metals like?

A

They must have roman numeral to indicate specifically which of them is bein talked about

147
Q

What are binary molecular compounds?

A

They are compounds formed by 2 non-metals

148
Q

What are acids?

A

They are binary molecular compounds having hydrogen which ionize in water to release H+ ions.

149
Q

Are acids called so when in gaseous form?

A

No, only when they are in Water.

150
Q

Oxoacids what are they?

A

They are acids with oxygen in addition to Hydrogen atoms.

151
Q

What are oxoanions?

A

Are polyatomic ions composed of an element, typically a nonmetal, bonded to one or more oxygen atoms. E.g NO3 (Nitrate)

152
Q

What are isobars?

A

Are the nuclei with the same mass number but different atomic numbers.

153
Q

What are Quantum numbers?

A

They are numbers used to describe the ENERGY LEVELS available to ELECTRONS in atoms.

154
Q

What are the WAVE FUNCTIONS of Certain QUANTUM NUMBERS associated with?

A

An electron

155
Q

What can the expression of the WAVE FUNCTION in these electrons help us know?

A
  • The ENERGY of the orbital
  • The SHAPE of the orbital
  • The ORIENTATION in space of the orbital
156
Q

How many QUANTUM NUMBERS does an Electron have?

A

4 of them. (n, l, ml & ms)

157
Q

What is the FIRST QUANTUM NUMBER?

A

It’s the PRINCIPAL ENERGY LEVEL of an atom. It is denoted by a small “n”

158
Q

What is special between HYDROGEN & the Principal energy level?

A

The Energy level depends only on “n”

159
Q

What does the bigger value of “n” means?

A

It means that the ENERGY OF THE ELECTRON is increasing, and it is found further from the NUCLEUS.

160
Q

What’s a Sub-level?

A

A sub-division of the first energy level, n

161
Q

What does the SECOND QUANTUM NUMBER, l give us?

A

It gives us the SHAPE of the cloud of electrons.

162
Q

What does LARGER VALUES of l denote?

A

They denote more complex shape of electrons in an atom

163
Q

What is the THIRD QUANTUM NUMBER, ml?

A

It’s the quantum number which determines the DIRECTION OF SPIN of the Electron Cloud in Space.

164
Q

What does the FOURTH QUANTUM Number tell us?

A

It tells us of the DIRECTION OF THE SPIN.

165
Q

What are the parallel spins?

A

The electrons with the same DIRECTION OF SPIN

166
Q

What are OPPOSITE SPINS?

A

Are the electrons with the OPPOSITE SPIN DIRECTION

167
Q

State the PAULI’S EXCLUSION PRINCIPLE:

A

No 2 electrons in an ATOM can have the SAME 4 Identical QUANTUM NUMBERS.

168
Q

What are some ways we can represent electrons?

A

Through QUANTUM Numbers, Orbitals & through electronic configuration & ORBITAL DIAGRAMS to name a few.

169
Q

What is an ELECTRONIC CONFIGURATION?

A

An electronic configuration is the way of representing electrons as populations in their respective Sub-levels.

170
Q

What is the abbreviated electronic configuration?

A

A notation of denoting electrons by shortening using a Noble gas which corresponds to the amount of number of electrons satisfying it

171
Q

What are ORBITAL DIAGRAMS?

A

A way to present electrons by showing ELECTRON SPINS directions as UP & DOWN ARROWS.

172
Q

State Hund’s RULE:

A

“When several Orbitals of Equal energy are available, as in a given SUB-LEVEL, electrons enter singly with Parallel Spins”

173
Q

What are PAIRED electrons in orbitals?

A

They are the ELECTRONS of OPPOSITE Spins occupying the Orbitals.

174
Q

What does PARAMAGNETIC mean?

A

It means showing magnetic attraction due to the presence of UNPAIRED ELECTRONS.

175
Q

What does DIMAGNETIC mean?

A

It means showing a REPULSION of a Magnetic FIELD, due to the presence of PAIRED ELECTRONS.

176
Q

What are Isoelectronic elements?

A

They are atoms with the same electronic configuration.

177
Q

Why do metals to the right of Scandium not form ions with noble gas configurations?

A

because it would require a lot of energy to remove the electrons.

178
Q

State the Periodic Law:

A

“The chemical & physical properties of elements are a periodic function of their atomic number”

179
Q

What is ATOMIC RADIUS?

A

It’s One half of the closest distance of the nuclei from an ordinary element

180
Q

What is ATOMIC RADIUS?

A

It’s half of the closest distance of the nuclei from an ordinary element. (Assumed Elements are connected)

181
Q

What’s the TREND OF THE ATOMIC RADII in the Periodic TABLE?

A
  • It INCREASES DOWN THE GROUP
  • It DECREASES ACROSS THE PERIOD
182
Q

What is IONIC RADIUS?

A

It’s the RADIUS assigned to a MONO-ATOMIC atom

183
Q

What’s the Trend of IONIC RADIUS in the PERIODIC Table?

A
  • It INCREASES DOWN THE GROUP
  • It DECREASES ACROSS THE PERIOD
184
Q

What is IONIZATION ENERGY?

A

It’s the measure of how diffciulty it is to REMOVE AN ELECTRON FROM A GASEOUS ATOM.

185
Q

What is IONIZATION ENERGY?

A

It measures how difficult it is to REMOVE AN ELECTRON FROM A GASEOUS ATOM.

186
Q

What is the FIRST IONIZATION ENERGY?

A

It is the ENERGY CHANGE for the removal of the OUTERMOST ELECTRON.

187
Q

What is the Trend for IONIZATION ENERGY in the PERIODIC Table?

A
  • It INCREASES ACROSS THE PERIOD
    -It DECREASES DOWN the GROUP
188
Q

What is ELECTRONEGATIVITY?

A

The tendency of an Atom to attract electrons towards itself/its bonds.

189
Q

What is Density?

A

it’s the unit mass of substance over equal volume of that substance

190
Q

What are the applications of density?

A
  • Floating of ship
  • Construction of aeroplane
  • Filling Balloon with air
  • The use of metals & metalloids in various bioprosthetics usages
191
Q

Why does ship float in water? or Submarine, or aeroplane?

A

The surface area & volume inside makes it later with it’s mass, that is less denser.

192
Q

Why do Balloons float in air?

A

Because the Hydrogen air in it becomes on top of the Balloon, making it to float.

193
Q

What specifically makes aeroplanes float in air?

A
  • The materials used in construction, & the fuel are all less denser. The materials are metalloids which are less denser
  • The air in space within
194
Q

What’s the difference between ACCURACY & PRECISION?

A

Accuracy - Means the closeness of the experimental value to the actual value.
Precision - The carryout of experiment/analysis to get closer to accurate value

195
Q

What’s the difference between ACCURACY & PRECISION?

A

Accuracy - This means the closeness of the experimental value to the actual value.
Precision - The closeness of the experimented values to themselves & tp the accurate value

196
Q

What is a PYCNOMETER?

A

It’s a Lab apparatus to determine density

197
Q

What’s a TETRAHEDRA?

A

A figure with 3 triangular faces and a triangular base

198
Q

What happens as electrons are at an optimum distance & energy?

A

It forms a MOLECULE State e.g in Hydrogen Molecule

199
Q

Where does COVALENT BOND Exist?

A

In the MOLECULES & POLYATOMIC IONS

200
Q

What’s the FUNDAMENTAL LOGIC BEHIND LEWIS Structure?

A

By sharing electrons, Non-metals become stable, as they acquire NOBLE GAS STRUCTURE.

201
Q

What are VALENCE ELECTRONS?

A

The electrons of the Outermost Principal energy “n”. For the Main Group elements it’s the last digit of the group number.

202
Q

What is a LEWIS STRUCTURE?

A

A structure of a molecule or an ion, Showing the bond and the electrons as dots surrounding the atoms.

203
Q

Why are the VALENCE Electrons only shown in the LEWIS STRUCTURE?

A

Because they are the one which participate in the Covalent bond

204
Q

What is an unshared electron pair?

A

It is a PAIR of electrons belonging to one ATOM. It isn’t involved in a BONDING

205
Q

What is a lone pair?

A

It is a pair of electrons that are unbonded and exists in a single atom

206
Q

What is a SINGLE BOND?

A

It is a bond consisting of only a SINGLE PAIR of shared electrons

207
Q

What is a DOUBLE BOND?

A

It is a bond consisting of TWO PAIRS of shared elctrons

208
Q

State the OCTET RULE:

A

Bonded atoms (Except Hydrogen), tend to have share in eight Valence electrons

209
Q

What’s a Central atom?

A

An atom at the centre of a MOLECULE, to which one or more electrons are bonded from

210
Q

What are Terminal atoms?

A

They are the atoms bonded to the CENTRAL ATOM. They are usually Hydrogen, Oxygen or Halogens

211
Q

Which atoms usually NEVER form Double BONDS?

A

Hydrogen & Halogens

212
Q

What separates REASONANCE STRUCTURES?

A

A double headed arrow

213
Q

What is a REASONANCE STRUCTURE/form?

A

A presentation of a Lewis structure of a molecule, showing the possibilities that the real structure might be one of them

214
Q

What is the REASONANCE HYBRID FORM?

A

The presentation of a Resonance structure.

215
Q

Why is RESONANCE there?

A

They occur when a Lewis structure fails to describe the real properties of a substance.

216
Q

Mention an organic Structure with REASONANCE

A

Benzene

217
Q

What are ISOMERS?

A

They are compounds with same formula but different properties

218
Q

What is the FORMAL CHARGE?

A

It is a charge that an ATOM will have in a molecule if the BONDING ELECTRONS were equally shared

219
Q

What are the applications of the FORMAL CHARGE?

A

It helps us know the CORRECT LEWIS STRUCTURE.

220
Q

What is the other name given to the Odd electron Species like NO?

A

Free Radicals

221
Q

What are FREE RADICALS?

A

They are the polyatomic ions which don’t OBEY THE LEWIS STRUCTURE, by having a deficiency in the Central atom

222
Q

What are the EXPANDED OCTETS?

A

They are the Species of compounds which have more than 8 electrons in their Central atom

223
Q

What are bond angles?

A

They are angles between 2 covalent Bonds

224
Q

What is a linear molecule?

A

A triatomic molecule with a bond angle of 180 degrees

225
Q

What’s a BENT MOLECULE?

A

A triatomic molecule with Bond Angles less than 180 degrees.

226
Q

What is Molecular Geometry?

A

The shape of the molecule showing the relative position of atoms

227
Q

What is Electron PAIR REPULSION?

A

The principle to predict the Shape of the molecule, where the atoms repel each other as far as possible

228
Q

What is VSEPR?

A

It’s the Valence Shell Electron Pair Repulsion Theory

229
Q

What does the VSEPR model suggest?

A

That the Valence electron pairs surrounding an atom repel one another and the Orbitals with these shells are oriented far apart from each other

230
Q

What is an IDEAL GEOMETRY?

A

It is the Geometry of the molecule assuming the effect of the Unshared electrons was neglected

231
Q

What are the Bond angles of Molecular geometry?

A
  • Linear = 180
  • Trigonal planar = 120
  • Tetrahedron = 109.5
  • Trigonal bipyramid = 90,120,180
  • Octahedron = 90, 180
232
Q

What is a Polar molecule?

A

A Covalent Bond molecule with UNSYMETRICAL distributions of electrons, hence forming a +ve & a -ve Pole (Dipole)

233
Q

What is a Non-Polar molecule?

A

A Covalent Bond molecule with SYMETRICAL distribution of electrons. Usually has no -ve or +ve Poles.

234
Q

What type of molecules have Non polar covalent Bonds?

A

Identical Atoms

235
Q

What is a DIPOLE MOMENT?

A

The extent to which the polar molecules orient themselves in an ELECTRIC FIELD

236
Q

What is a DIPOLE?

A

State at which a molecule has +ve & -ve poles in its atom

237
Q

Valence Bond Model

A

Models of the Electronic Structure of molecules in which electrons are assigned to ORBITALS. Whether Pure or hybridized of Individual atoms

238
Q

What is a hybridized atomic Orbital?

A

An orbital is formed by mixing 2 types of Orbitals

239
Q

What is HYBRIDIZATION?

A

It’s the mixing of 2 or more Orbitals or structures

240
Q

What is a Sigma Bond?

A

A chemical Bond which the Electron density in the Inter-Nuclear axis is High

241
Q

How is the Electron density along the Bonding axis of a Sigma Bond?

A

Along the axis, the Electron Density is zero

242
Q

What is a Pi Bond?

A

The chemical Bond in which the electron density is concentrated far off the Nuclear axis

B.Sc in Biomedical Engineering (4 decks)

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