Water Flashcards

Polar covalent bonds in water molecules result in hydrogen bonding. Four emergent properties of water contribute to Earth's suitability for life. Acidic and basic conditions affect living organisms

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1
Q

Polar Covalent Bonds

A

A covalent bond between atoms that differ in electronegativity. The shared electrons are pulled closer to the more electronegative atom, making it slightly negative and the other atom slightly positive

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2
Q

Polar Molecule

A

A molecule (such as water) with an uneven distribution of charges in different regions of the molecule

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3
Q

Cohesion

A

The linking together of like molecules, often by hydrogen bonds

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4
Q

Adhesion

A

The clinging of one substance to another, such as water to plant cell walls by means of hydrogen bonds

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5
Q

Surface Tension

A

A measure of how difficult it is to to stretch or break the surface of a liquid. Water has a high one because of the hydrogen bonding of surface molecules

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6
Q

Kinetic Energy

A

The energy associated with the relative motion of objects. Moving matter can perform work by imparting motion to other matter

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7
Q

Thermal Energy

A

Kinetic energy due to the random motion of atoms and molecules; energy in its most random form

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8
Q

Temperature

A

A measure in degrees of the average kinetic energy (thermal energy) of the atoms and molecules in a body of matter

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9
Q

Heat

A

Thermal energy in transfer from one body of matter to another

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10
Q

Calorie (cal)

A

The amount of heat energy required to raise the temperature of 1g of water by 1*C. The Calorie (with a capital C), usually used to indicate the energy content of food, is a kilocalorie

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11
Q

Kilocalorie (kcal)

A

A thousand calories; the amount of heat energy required to raise the temperature of 1kg of water by 1*C

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12
Q

Joule (J)

A

A unit of energy: 1J=0.239cal; 1cal=4.184J

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13
Q

Specific Heat

A

The amount of heat that must be absorbed or lost for 1g of a substance to change its temperature by 1*C

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14
Q

Heat of Vaporization

A

The quantity of heat a liquid must absorb for 1g of it to be converted from the liquid to the gaseous state

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15
Q

Evaporative Cooling

A

The process in which the surface of an object becomes cooler during evaporation, a result of the molecules with the greatest kinetic energy changing from the liquid to the gaseous state

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16
Q

Solution

A

A liquid that is a homogeneous mixture of two or more substances

17
Q

Solvant

A

The dissolving agent of a solution. Water is the most versatile one known

18
Q

Solute

A

A substance that is dissolved in a solution

19
Q

Aqueous Solution

A

A solution in which water is the solvant

20
Q

Hydration Shell

A

The sphere of water molecules around a dissolved ion

21
Q

Hydrophilic

A

Having an affinity for water

22
Q

Hydrophobic

A

Having no affinity for water; tending to coalesce and form droplets in water

23
Q

Molecular Mass

A

The sum of the masses of all the atoms in a molecule; sometimes called the molecular weight

24
Q

Mole (mol)

A

The number of grams of a substance that equals its molecular or atomic mass in daltons; this contains Avogadro’s number of the molecules or atoms in question

25
Q

Molarity

A

A common measure of solute concentration, referring to the number of moles of solute per liter of solution

26
Q

Hydrogen Ion

A

A single proton with a charge of 1+. The dissociation of a water molecule (H2O) leads to the generation of a hydroxide ion (OH-) and a hydrogen ion (H+); in water, H+ is not found alone but associates with a water molecule to form a hydronium ion

27
Q

Hydroxide Ion

A

A water molecule that has lost a proton; OH-

28
Q

Hydronium Ion

A

A water molecule that has an extra proton bound to it; H30+, commonly represented as H+

29
Q

Acid

A

A substance that increases the hydrogen ion concentration of a solution

30
Q

Base

A

A substance that reduces the hydrogen ion concentration of a solution

31
Q

pH

A

A measure of hydrogen ion concentration equal to -log[H+] and ranging in value from 0 to 14

32
Q

Buffer

A

A solution that contains a weak acid and its corresponding base. This minimizes changes in pH when acids or bases are added to the solution

33
Q

Ocean Acidification

A

Decreasing pH of ocean waters due to absorption of excess atmospheric CO2 from the burning of fossil fuels