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Chapter 3 Water and Life Key Concepts

Chapter 3 Water and Life Key Concepts. Polar __________ bonds in water molecules result in __________ bonding Four emergent properties of __________ contribute to Earths suitability for __________ __________ and __________ conditions affect living organisms.

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Chapter 3 Water and Life Key Concepts

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  1. Chapter 3 Water and LifeKeyConcepts • Polar __________ bonds in water molecules result in __________ bonding • Four emergent properties of __________ contribute to Earths suitability for __________ • __________ and __________ conditions affect living organisms

  2. Chapter 3 Water and LifeKeyConcepts • Polar covalent bonds in water molecules result in hydrogen bonding • Four emergent properties of water contribute to Earths suitability for life • Acidic and basic conditions affect living organisms

  3. Oxygen is more __________ than hydrogen

  4. Oxygen is more electronegative than hydrogen

  5. __________ bonds are about 1/20 the strength of __________ bonds.

  6. Hydrogen bonds are about 1/20 the strength of covalent bonds.

  7. 4 emergent properties of water • ____________ due to hydrogen bonding • Moderation of ____________ by water • Floating of ____________ on liquid water • Water: The ____________ of life

  8. 4 emergent properties of water • Cohesion due to hydrogen bonding • Moderation of temperature by water • Floating of ice on liquid water • Water: The solvent of life

  9. Water transport in plants is an example of ____________ and ____________ ____________ ____________ in water is an example of a property due to hydrogen bonding

  10. Water transport in plants is an example of cohesion and adhesion Surface tension in water is an example of a property due to hydrogen bonding

  11. __________ is total kinetic energy of the molecules of a body – it depends on __________ and is measured in __________ , __________ or __________ __________ is a measure of the __________ kinetic energy and is measured in degrees ___________

  12. Heat is total kinetic energy of the molecules of a body – it depends on volume and is measured in calories, kilocalories or joules Temperature is a measure of the average kinetic energy and is measured in degrees Celsius

  13. The material property __________ __________ is the number of __________ to raise 1 gram of the material by __________ __________

  14. The material property Specific Heat is the number of Calories to raise 1 gram of the material by 1° C

  15. Water’s relatively _______ specific heat is due to _______ _______ Water temperature _______ slowly when heat is applied because the heat is first used to break _______ _______ then is used to _______ the _______ of molecules

  16. Water’s relatively high specific heat is due to hydrogen bonding Water temperature rises slowly when heat is applied because the heat is first used to break hydrogen bonds then is used to increase motion of molecules

  17. Heat of __________ is the heat needed to convert 1 gm of __________ to vapor This parameter for water is _________ calories

  18. Heat of vaporization is the heat needed to convert 1 gm of liquid to vapor This parameter for water is 580 calories

  19. Heat added to water during _________ _________ ocean water temperature Heat released from water vapor during _________ in the upper atmosphere _________ atmospheric temperature

  20. Heat added to evaporating water during evaporation comes from the water left behind, and lowers ocean water temperature Heat released during condensation back to liquid form in the upper atmosphere raises atmospheric temperature

  21. At 0°C hydrogen bonds lock in a __________ lattice becoming __________ Hydrogen bonds in ice are __________ apart than they are in __________ at 4°C

  22. At 0°C hydrogen bonds lock in a crystalline lattice becoming ice Hydrogen bonds in ice are further apart than they are in water at 4°C

  23. 2 or more substances dissolved in a liquid is called a _________. The dissolving liquid is called a _________. The dissolved substance is called a _________. When the solvent is water the solution is called ________.

  24. 2 or more substances dissolved in a liquid is called a solution. The dissolving liquid is called a solvent. The dissolved substance is called a solute. When the solvent is water the solution is called aqueous.

  25. When salt is dissolved in water • _______ _______ are plucked off by the O- side of H2O molecules • _______ _______ are plucked off by the H+ side of H2O molecules • The resulting water molecule wrapper around the cations and anions is called a _______ shell

  26. When salt is dissolved in water • Sodium cations are plucked off by the O- side of H2O molecules • Cloride anions are plucked off by the H+ side of H2O molecules • The resulting water molecule wrapper around cations and anions is called a hydration shell

  27. A mole is _______ molecules • A mole of a particular compound weighs its molecular weight in _______ • H2O weighs _________ grams/mole • ______ weighs 22.99 + 35.45 = 58.44 gms/mole • Put 58.44 gms of NaCl in 1 liter of H2O and it is a 1 _____ (1M) solution of NaCl

  28. A mole is 6.02 x 1023 molecules • A mole of a particular compound weighs its molecular weight in grams • H2O weighs 1+1+16 = 18 grams/mole • NaCl weighs 22.99 + 35.45 = 58.44 gms/mole • Put 58.44 gms of NaCl in 1 liter of H2O and it is a 1 molar (1M) solution of NaCl

  29. When hydrogen bonds go bad • Water that loses 1 H proton (but not the electron) is OH- and is called a _________ ion • Water that gains the proton is H3O+ and is called a _________ ion, usually denoted by just _________ • Equal amounts of hydroxide and hydronium are in pure _________

  30. When hydrogen bonds go bad • Water that loses 1 H proton (but not the electron) is OH- and is called a hydroxide ion • Water that gains the proton is H3O+ and is called a hydronium ion, usually denoted by just H+ • Equal amounts of hydroxide and hydronium are in pure water

  31. When _______dissolve in water they donate additional ___ ___ ( which becomes H3O+) _____lower pH 2 ways: • Accepting H+ (NH3, ammonia, attracts a _______to its unbonded electron pair) • Donating ___ ___ ___ (NaOH-> Na+ and OH-) H N H H+ H

  32. When acids dissolve in water they donate additional H+ ( which becomes H3O+) Bases lower pH 2 ways: • Accepting H+ (NH3, ammonia, attracts a proton to its unbonded electron pair) • Donating OH- (NaOH-> Na+ and OH-) H N H H+ H

  33. In ______acids and bases the disassociation equation arrow goes one way NaOH Na+ and OH- • In ______acids and bases the disassociation equation arrow goes both ways H2CO3 HCO3- and H+

  34. In strong acids and bases the disassociation equation arrow goes one way NaOH Na+ and OH- • In weak acids and bases the disassociation equation arrow goes both ways H2CO3 HCO3- and H+

  35. [ H+] [OH-] = _____

  36. [ H+] [OH-] = 10-14

  37. _____ stability is assisted by ______ in blood an important one is _________ acid H2CO3 <====> _______ and _____

  38. pH stability is assisted by buffers in blood an important one is carbonic acid H2CO3 <====> HCO3- and H+

  39. In an abnormally _____ocean H+ combines with ________ ions, CO32- to make bicarbonate, robbing _______of the CO32- they use to grow.

  40. In an abnormally acidic ocean H+ combines with carbonate ions, CO32- to make bicarbonate, robbing corals of the CO32- they use to grow.

  41. END OF CHAPTER 3

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