Physiology MCQs
1. Unit of distensibility is
a) ml/mmHg ✅
b) mmHg ml
c) mmHg/ml
2. The Compliance of veins to arteries
a) 8 times
b) 16 times
c) 24 times✅
3. The pulmonary artery pressure as compared to systemic arterial pressure is
a) 1/10th
b) 1/6th ✅
c) 1/3rd
4. Distensibility is
a) Compliance/volume ✅
b) Volume/ Compliance
c) Compliance * Volume
5. When blood is 400 ml in arterial system, then pressure is
a) 700 mmHg
b) 0 mmHg ✅
c) 100 mmHg
6. The Circulation compensated even if blood loss is
a) 25% ✅
b) 20%
c) 15%
7. Delayed compliance occurs in
a) Arteries
b) Veins ✅
c) Arterioles
8. Pulse Pressure is
a) Compliance / Stroke volume
b) compliance * stroke volume
c) stroke vol / compliance✅
9. Arterial pressure depends upon
a) stroke vol
b) compliance
c) Both a & b✅
10. Pressure and compliance relationship is
a) Direct
b) Inverse✅
c) None of these
1. Unit of distensibility is
a) ml/mmHg ✅
b) mmHg ml
c) mmHg/ml
2. The Compliance of veins to arteries
a) 8 times
b) 16 times
c) 24 times✅
3. The pulmonary artery pressure as compared to systemic arterial pressure is
a) 1/10th
b) 1/6th ✅
c) 1/3rd
4. Distensibility is
a) Compliance/volume ✅
b) Volume/ Compliance
c) Compliance * Volume
5. When blood is 400 ml in arterial system, then pressure is
a) 700 mmHg
b) 0 mmHg ✅
c) 100 mmHg
6. The Circulation compensated even if blood loss is
a) 25% ✅
b) 20%
c) 15%
7. Delayed compliance occurs in
a) Arteries
b) Veins ✅
c) Arterioles
8. Pulse Pressure is
a) Compliance / Stroke volume
b) compliance * stroke volume
c) stroke vol / compliance✅
9. Arterial pressure depends upon
a) stroke vol
b) compliance
c) Both a & b✅
10. Pressure and compliance relationship is
a) Direct
b) Inverse✅
c) None of these
🔥🔥Notes on Chemical Bonding🔥🔥
©™✓✓✓✓✓✓✓✓✓✓✓✓✓
🔻Chemical bond:-
Chemical bond is the attractive force which holds various constituents together in a molecule.
There are three types of chemical bonds: Ionic Bond, Covalent Bond, Co-ordinate Bond.
🔻Octet Rule:
Atoms form chemical bonds in order to complete their octet i.e. eight electrons in their valence shell.
🔥Lewis Structures:
Pair of bonded electrons is by means of a ‘dash’ (-) usually called a ‘bond’.
Lone pairs or ‘non-bonded’ electrons are represented by ‘dots’.
Electrons present in the last shell of atoms are called valence electrons.
✌️Exceptions to the Octet Rule:
🔻Species with odd number of electrons: NO, NO2,
🔻Incomplete octet for the central atom: LiCl, BeH2 and BCl3
🔻Expanded octet for the central atom: PF5, SF6 and H2SO4
🔻Formal Charge:
Formal charge is the difference between the number of valence electrons in an isolated atom and number of electrons assigned to that atoms in Lewis structure.
Formal charge = [Total number of valence electrons in the free atom ) - (Total number of lone pairs of electrons) -1/2(Total number of shared electrons i.e. bonding electrons)]
🔥Resonance:
For molecules and ions showing resonance it is not possible to draw a single Lewis structure.
All the properties of such species can only be explained by two or more Lewis structures. Example: Resonance of O3
🔥Ionic Bonding:
🔻Formation of Ionic Bond:
Formation of ionic bond takes place between a metal and a non-metal by transfer of electron.
Formation of gaseous cations
A(g) + I.E. → A+ (g) + e
🔥Ionization Energy
Formation of gaseous anions
X(g) + e → X- (g) + E.A
🔥Electron Affinity
Packing of ions of opposite charges to form ionic solids
A+ (g) + X- (g) →AX (s) +Energy
🔥Lattice energy
Conditions required of formation of ionic bonds:
🔻Low I.E of cation.
🔻High E.A of anion.
🔻High lattice energy.
⚡Covalent Bonding:
Covalent bond is formed between two non-metals by sharing of electrons.
🔻Electron pairs which participate in bonding are called bond pairs.
🔻Electron pairs which do not participate in bonding are called lone pairs.
There could be single, double or triple covalent bonds between two elements depending on the number of electrons being shared.
🔥VSEPR (Valence Shell Electron Pair Repulsion) Theory:
The shape of the molecule is determined by repulsions between all of the electron pairs present in the valence shell.
🔻Order of the repulsion: Lone pair.Lone pair > Lone pair. Bond pair > Bond pair. Bond pair.
🌡️Repulsion among the bond pairs is directly proportional to the bond order and electronegativity difference between the central atom and the other atoms.
©™✓✓✓✓✓✓✓✓✓✓✓✓✓
🔻Chemical bond:-
Chemical bond is the attractive force which holds various constituents together in a molecule.
There are three types of chemical bonds: Ionic Bond, Covalent Bond, Co-ordinate Bond.
🔻Octet Rule:
Atoms form chemical bonds in order to complete their octet i.e. eight electrons in their valence shell.
🔥Lewis Structures:
Pair of bonded electrons is by means of a ‘dash’ (-) usually called a ‘bond’.
Lone pairs or ‘non-bonded’ electrons are represented by ‘dots’.
Electrons present in the last shell of atoms are called valence electrons.
✌️Exceptions to the Octet Rule:
🔻Species with odd number of electrons: NO, NO2,
🔻Incomplete octet for the central atom: LiCl, BeH2 and BCl3
🔻Expanded octet for the central atom: PF5, SF6 and H2SO4
🔻Formal Charge:
Formal charge is the difference between the number of valence electrons in an isolated atom and number of electrons assigned to that atoms in Lewis structure.
Formal charge = [Total number of valence electrons in the free atom ) - (Total number of lone pairs of electrons) -1/2(Total number of shared electrons i.e. bonding electrons)]
🔥Resonance:
For molecules and ions showing resonance it is not possible to draw a single Lewis structure.
All the properties of such species can only be explained by two or more Lewis structures. Example: Resonance of O3
🔥Ionic Bonding:
🔻Formation of Ionic Bond:
Formation of ionic bond takes place between a metal and a non-metal by transfer of electron.
Formation of gaseous cations
A(g) + I.E. → A+ (g) + e
🔥Ionization Energy
Formation of gaseous anions
X(g) + e → X- (g) + E.A
🔥Electron Affinity
Packing of ions of opposite charges to form ionic solids
A+ (g) + X- (g) →AX (s) +Energy
🔥Lattice energy
Conditions required of formation of ionic bonds:
🔻Low I.E of cation.
🔻High E.A of anion.
🔻High lattice energy.
⚡Covalent Bonding:
Covalent bond is formed between two non-metals by sharing of electrons.
🔻Electron pairs which participate in bonding are called bond pairs.
🔻Electron pairs which do not participate in bonding are called lone pairs.
There could be single, double or triple covalent bonds between two elements depending on the number of electrons being shared.
🔥VSEPR (Valence Shell Electron Pair Repulsion) Theory:
The shape of the molecule is determined by repulsions between all of the electron pairs present in the valence shell.
🔻Order of the repulsion: Lone pair.Lone pair > Lone pair. Bond pair > Bond pair. Bond pair.
🌡️Repulsion among the bond pairs is directly proportional to the bond order and electronegativity difference between the central atom and the other atoms.
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Notes on Chemical Bonding
🔻Chemical bond:-
Chemical bond is the attractive force which holds various constituents together in a molecule.
There are three types of chemical bonds: Ionic Bond, Covalent Bond, Co-ordinate Bond.
🔻Octet Rule:
Atoms form chemical bonds in order to complete their octet i.e. eight electrons in their valence shell.
🔥Lewis Structures:
Pair of bonded electrons is by means of a ‘dash’ (-) usually called a ‘bond’.
Lone pairs or ‘non-bonded’ electrons are represented by ‘dots’.
Electrons present in the last shell of atoms are called valence electrons.
✌️Exceptions to the Octet Rule:
🔻Species with odd number of electrons: NO, NO2,
🔻Incomplete octet for the central atom: LiCl, BeH2 and BCl3
🔻Expanded octet for the central atom: PF5, SF6 and H2SO4
🔻Formal Charge:
Formal charge is the difference between the number of valence electrons in an isolated atom and number of electrons assigned to that atoms in Lewis structure.
Formal charge = [Total number of valence electrons in the free atom ) - (Total number of lone pairs of electrons) -1/2(Total number of shared electrons i.e. bonding electrons)]
🔥Resonance:
For molecules and ions showing resonance it is not possible to draw a single Lewis structure.
All the properties of such species can only be explained by two or more Lewis structures. Example: Resonance of O3
🔥Ionic Bonding:
🔻Formation of Ionic Bond:
Formation of ionic bond takes place between a metal and a non-metal by transfer of electron.
Formation of gaseous cations
A(g) + I.E. → A+ (g) + e
🔥Ionization Energy
Formation of gaseous anions
X(g) + e → X- (g) + E.A
🔥Electron Affinity
Packing of ions of opposite charges to form ionic solids
A+ (g) + X- (g) →AX (s) +Energy
🔥Lattice energy
Conditions required of formation of ionic bonds:
🔻Low I.E of cation.
🔻High E.A of anion.
🔻High lattice energy.
⚡Covalent Bonding:
Covalent bond is formed between two non-metals by sharing of electrons.
🔻Electron pairs which participate in bonding are called bond pairs.
🔻Electron pairs which do not participate in bonding are called lone pairs.
There could be single, double or triple covalent bonds between two elements depending on the number of electrons being shared.
🔥VSEPR (Valence Shell Electron Pair Repulsion) Theory:
The shape of the molecule is determined by repulsions between all of the electron pairs present in the valence shell.
🔻Order of the repulsion: Lone pair.Lone pair > Lone pair. Bond pair > Bond pair. Bond pair.
🌡️Repulsion among the bond pairs is directly proportional to the bond order and electronegativity difference between the central atom and the other atoms.
🔻Chemical bond:-
Chemical bond is the attractive force which holds various constituents together in a molecule.
There are three types of chemical bonds: Ionic Bond, Covalent Bond, Co-ordinate Bond.
🔻Octet Rule:
Atoms form chemical bonds in order to complete their octet i.e. eight electrons in their valence shell.
🔥Lewis Structures:
Pair of bonded electrons is by means of a ‘dash’ (-) usually called a ‘bond’.
Lone pairs or ‘non-bonded’ electrons are represented by ‘dots’.
Electrons present in the last shell of atoms are called valence electrons.
✌️Exceptions to the Octet Rule:
🔻Species with odd number of electrons: NO, NO2,
🔻Incomplete octet for the central atom: LiCl, BeH2 and BCl3
🔻Expanded octet for the central atom: PF5, SF6 and H2SO4
🔻Formal Charge:
Formal charge is the difference between the number of valence electrons in an isolated atom and number of electrons assigned to that atoms in Lewis structure.
Formal charge = [Total number of valence electrons in the free atom ) - (Total number of lone pairs of electrons) -1/2(Total number of shared electrons i.e. bonding electrons)]
🔥Resonance:
For molecules and ions showing resonance it is not possible to draw a single Lewis structure.
All the properties of such species can only be explained by two or more Lewis structures. Example: Resonance of O3
🔥Ionic Bonding:
🔻Formation of Ionic Bond:
Formation of ionic bond takes place between a metal and a non-metal by transfer of electron.
Formation of gaseous cations
A(g) + I.E. → A+ (g) + e
🔥Ionization Energy
Formation of gaseous anions
X(g) + e → X- (g) + E.A
🔥Electron Affinity
Packing of ions of opposite charges to form ionic solids
A+ (g) + X- (g) →AX (s) +Energy
🔥Lattice energy
Conditions required of formation of ionic bonds:
🔻Low I.E of cation.
🔻High E.A of anion.
🔻High lattice energy.
⚡Covalent Bonding:
Covalent bond is formed between two non-metals by sharing of electrons.
🔻Electron pairs which participate in bonding are called bond pairs.
🔻Electron pairs which do not participate in bonding are called lone pairs.
There could be single, double or triple covalent bonds between two elements depending on the number of electrons being shared.
🔥VSEPR (Valence Shell Electron Pair Repulsion) Theory:
The shape of the molecule is determined by repulsions between all of the electron pairs present in the valence shell.
🔻Order of the repulsion: Lone pair.Lone pair > Lone pair. Bond pair > Bond pair. Bond pair.
🌡️Repulsion among the bond pairs is directly proportional to the bond order and electronegativity difference between the central atom and the other atoms.
Aluminium metal is extracted mainly from its ore :
Anonymous Poll
24%
Magnetite
67%
Bauxite
9%
Dolomite
1%
Lime pigment
✌️IMP OF PLANT KINGDOM✌️
👉Isogamous sexual reproduction in algae- Ulothrix (flagellated)
Spirogyra (non-flagellated)
👉Anisogamous sexual reproduction in algae- Udorina
👉Oogamous sexual reproduction in algae- Volvox, Fucus
👉Algin- Brown Algae
👉Carragreen - Red Algae
👉Agar- Gelidium, Gracilaria
(Red algae)
👉Motile asexual spores in algae- Zoospores
👉Laminarin, Mannitol- Complex carbohydrates of Brown algae
👉Fucoxanthin- Brown Algae
👉Phycoerythrin- Red Algae
👉Floridean Starch Found in Red algae, similar to amylopectin and glycogen
👉The main plant body is a gametophyte- Bryophytes
👉Peat- Sphagnum
👉Microphylls- Selaginella
👉Macrophylls- Fern
👉Isogamous sexual reproduction in algae- Ulothrix (flagellated)
Spirogyra (non-flagellated)
👉Anisogamous sexual reproduction in algae- Udorina
👉Oogamous sexual reproduction in algae- Volvox, Fucus
👉Algin- Brown Algae
👉Carragreen - Red Algae
👉Agar- Gelidium, Gracilaria
(Red algae)
👉Motile asexual spores in algae- Zoospores
👉Laminarin, Mannitol- Complex carbohydrates of Brown algae
👉Fucoxanthin- Brown Algae
👉Phycoerythrin- Red Algae
👉Floridean Starch Found in Red algae, similar to amylopectin and glycogen
👉The main plant body is a gametophyte- Bryophytes
👉Peat- Sphagnum
👉Microphylls- Selaginella
👉Macrophylls- Fern
1: Anti Histamine = Use in Allergy
2: Analgesic = Pain Killer
3: Anti Pyretic = Fever
4: Anti Septic = Pus
5: Anti Biotic = Infection
6: Anti Anaemia = Low blood
7: Anti Emetic = Vomting
8: Anti Acid = Stomach Burn
9: Anti Flantulents = Gases
10: Anti Spasmodic = Abdominal pain
11: Anti Anginal = Cardiac pain
12: Anti Arhthnic = Cardiac Activity
13: Ant Hypertensive = BP
14: Anti Lipemic = Chlosterol+Lipids
15: Anti Coagulant = Norrowing of Blood
16: Anti Depressant = Depression
17: HYPONOTIC = For Sleep
18: Anti Psychotic = For Psychosis
19: Anti Anxiety = For Anxiety
20: Anti Parkinson = For Parkinson's
2: Analgesic = Pain Killer
3: Anti Pyretic = Fever
4: Anti Septic = Pus
5: Anti Biotic = Infection
6: Anti Anaemia = Low blood
7: Anti Emetic = Vomting
8: Anti Acid = Stomach Burn
9: Anti Flantulents = Gases
10: Anti Spasmodic = Abdominal pain
11: Anti Anginal = Cardiac pain
12: Anti Arhthnic = Cardiac Activity
13: Ant Hypertensive = BP
14: Anti Lipemic = Chlosterol+Lipids
15: Anti Coagulant = Norrowing of Blood
16: Anti Depressant = Depression
17: HYPONOTIC = For Sleep
18: Anti Psychotic = For Psychosis
19: Anti Anxiety = For Anxiety
20: Anti Parkinson = For Parkinson's
🍒BORON:
•In casting of copper as a dioxidizer
•Boron rods used in automic reactor.
•Boron fiber used in bullet proof jacket,
•In composite material of aircraft
•Used in braintumer therapy.
🍒 BORAX:
•As a flux for soldring metal.
•In borex bead test
•In softning of water
•Antiseptic
•Manufacturing of enamels of glazes, tiles.
•For making optical and borosilicals SS.
•Food preservative
🍒 ALUMINIUM:
• Making house hold, untensils, frames, roof,aircrafts.
• Electric wire.
•Thermite process (In metallurgy of Cr, Mn, Fe)
•For transportin nitric acid.
•AI, Hg used as reducing agent.
•Aluminium powder + Ammonium nitrate.
🍒 LEAD [Pb]:
•In making telegraph and telephone wires
•Making bullets
•Making chamber in HSO, process.
🍒 NITROGEN:
•In the manufacturing of HNO3, NH3, CaCN2.
•Liquid nitrogen used as refrigrant.
•Inert atmosphere in metallurgy.
•Gas thermometer and electrical bulb
🍒 NH3:
• Refrigeration
•Manufacturing HNO3, NaHCO3
•Artificial Silk.
• Urea Formation
•For solvent
🍒 HNO3:
• Manufacturing of ammonium nitrateas fertilizer.
•In explosive
• For making nitroglycerine.
• Making TNT.
• Pickling against of stainless steel.
• Etching of Metal
•Oxidizer in rocket fule.
•In casting of copper as a dioxidizer
•Boron rods used in automic reactor.
•Boron fiber used in bullet proof jacket,
•In composite material of aircraft
•Used in braintumer therapy.
🍒 BORAX:
•As a flux for soldring metal.
•In borex bead test
•In softning of water
•Antiseptic
•Manufacturing of enamels of glazes, tiles.
•For making optical and borosilicals SS.
•Food preservative
🍒 ALUMINIUM:
• Making house hold, untensils, frames, roof,aircrafts.
• Electric wire.
•Thermite process (In metallurgy of Cr, Mn, Fe)
•For transportin nitric acid.
•AI, Hg used as reducing agent.
•Aluminium powder + Ammonium nitrate.
🍒 LEAD [Pb]:
•In making telegraph and telephone wires
•Making bullets
•Making chamber in HSO, process.
🍒 NITROGEN:
•In the manufacturing of HNO3, NH3, CaCN2.
•Liquid nitrogen used as refrigrant.
•Inert atmosphere in metallurgy.
•Gas thermometer and electrical bulb
🍒 NH3:
• Refrigeration
•Manufacturing HNO3, NaHCO3
•Artificial Silk.
• Urea Formation
•For solvent
🍒 HNO3:
• Manufacturing of ammonium nitrateas fertilizer.
•In explosive
• For making nitroglycerine.
• Making TNT.
• Pickling against of stainless steel.
• Etching of Metal
•Oxidizer in rocket fule.
Important Points For NEET 🌟
Evidences from comparative morphology and anatomy :-
⚡️Examples of homologous organs:⚡️
(i) Forelimbs of mammals
(ii) Thorn of Bougainvillea and tendril of Cucurbita both are modification of axillary bud.
(iii)Vertebrate hearts or brains
(iv)Mouth parts of insects :
Cockroach Honey bee Mosquito
(Biting & chewing) (Chewing & lapping) (Piercing & Sucking)
(v) Testes in male and ovaries in female
(vi) Potato and Ginger - both are modified shoot
(vii) Radish and Carrot - both are modified roots
⚡️Examples of Analogous organs :⚡️
(i) Wings of butterfly and birds
(ii) Eye of the octopus and of mammals
(iii) Flippers of Penguins and Dolphins
(iv) Sweet potato (root modification) and potato (stem modification)
(v) Sting of bee and scorpion
(vi) Chloragogen cells of earthworm and liver of vertebrates
Evidences from comparative morphology and anatomy :-
⚡️Examples of homologous organs:⚡️
(i) Forelimbs of mammals
(ii) Thorn of Bougainvillea and tendril of Cucurbita both are modification of axillary bud.
(iii)Vertebrate hearts or brains
(iv)Mouth parts of insects :
Cockroach Honey bee Mosquito
(Biting & chewing) (Chewing & lapping) (Piercing & Sucking)
(v) Testes in male and ovaries in female
(vi) Potato and Ginger - both are modified shoot
(vii) Radish and Carrot - both are modified roots
⚡️Examples of Analogous organs :⚡️
(i) Wings of butterfly and birds
(ii) Eye of the octopus and of mammals
(iii) Flippers of Penguins and Dolphins
(iv) Sweet potato (root modification) and potato (stem modification)
(v) Sting of bee and scorpion
(vi) Chloragogen cells of earthworm and liver of vertebrates
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