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Chemistry > Intro > Flashcards

Intro Flashcards

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1
Q

Explain matter

A

Anything with mass and occupies space

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2
Q

Explain molecule

A

Smallest partial of a pure substance that has properties of that substance and is capable of a STABLE INDEPENDENT EXISTENCE

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3
Q

Explain atom

A

Is the limit of a chemical subdivision of a molecule

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4
Q

What’s an homoatomic molecule

A

The stable, independent form of elements i.e. o2

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5
Q

What’s a heteroatomic molecule

A

Stable independent COMPOUNDS i.e. co2

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6
Q

What’s homogeneous

A

Solution

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7
Q

What’s heterogeneous

A

Matter in this form i.e. Sand, gravel or a tomato

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8
Q

1 inch = ? Cm

A

2.54

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9
Q

Volume

A

Cubed, height x width x length

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10
Q

1 liter = ? cm

A

1000 cm(3) third power

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11
Q

1 cm(3) third power = ? mL

A

1 mL

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12
Q

1 teaspoon = ? mL

A

5 mL

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13
Q

1 fluid ounce = ? mL

A

30 mL

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14
Q

1 quart = ? mL

A

947 mL

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15
Q

1 pound = ? Grams

A

454 g

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16
Q

1 kg (killogram) = ? Lbs

A

2.2 lbs

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17
Q

Conversation for Fahrenheit to Celsius

A

F= 1.8 x (C) + 32

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18
Q

Def of calorie

Small c

A

The amount of energy required to raise the temperature of one centimeter cubed of water, one degree Celsius

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19
Q

Define element

A

Element molecules are homoatomic molecules, molecules with only one kind of atom
i.e. Helium= He or hydrogen=H

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20
Q

Define compound

A

Pure substances made up of two or more different kinds of atoms i.e. h2o, there are two hydrogen atoms and one oxygen atom

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21
Q

What’s an isotope

A

Atoms of same element whose nuclei contain different numbers of neutrons

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22
Q

What is the atomic number

A

Number of protons

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23
Q

What is the mass number

A

Total number of protons plus neutrons in nucleus

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24
Q

What’s an ion

A

An unequal amount of protons and electrons

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25
Q

One mole is equal to

A

6.022 x 10(23) power

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26
Q

4 shell types

A

s, p, d, f

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27
Q

Explain covalent bond

A

Strongest bond i.e. H2 and 02 and methane CH4

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28
Q

Explain polar covalent bonds

A

Slightly weaker than covalent, the molecule has positive and weaker side i.e. H2O

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29
Q

What’s an ionic bond

A

Electron is not really shared but taken to one side of the bond, causing a negatively charged ion and a positively charged ion on opposite sides of the bond i.e. Salt sodium chloride NaCl

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30
Q

Hydrogen bonding

A

Weakest of the bonds i.e. Water h2o and h2o

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31
Q

Molarity can be defined

A

The number of moles of solute per liter of solvent

I.e. 3 moles of sodium chloride dissolved in 2 liters of water is 3 moles divided by 2 liters equals 1.5 M

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32
Q

Osmole

A

1 mole of salt= 2 osmoles

1 mole of nonsalt= 1 osmole

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33
Q

Osmolartity

A

Osmoles of solute per liter of solvent,, milliosmoles (mOsm/L)

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34
Q

Mole

A

6.022 x 10(23)

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35
Q

Obital subshells have capacity of holding how many electrons

A

2

36
Q

Shell 1 has how many subshells/orbitals

A

One S, capacity two electrons

37
Q

Valence shell

A

Outermost shell, 4th subshell
Positive valence atoms are cations
Negative valence atoms become anions
F has 7 orbitals

38
Q

Noble gases react or don’t react

A

Don’t react w anything

39
Q

H

A

Hydrogen

40
Q

Li

A

Lithium

41
Q

C

A

Carbon

42
Q

He

A

Helium

43
Q

N

A

Nitrogen

44
Q

O

A

Oxygen

45
Q

Na

A

Sodium

46
Q

Mg

A

Magnesium

47
Q

P

A

Phosphorus

48
Q

Cl

A

Chlorine

49
Q

Ar

A

Argon

50
Q

K

A

Potassium

51
Q

Ca

A

Calcium

52
Q

Fe

A

Iron

53
Q

Calculating osmolarity

A

1.11 mole of glucose divided by liters

1 liter SOLUTION

54
Q

HCl

A

Hydrogen chloride

55
Q

Saturated solution

A

A solution that has reached solubility

56
Q

Immiscible

A

Applies to liquids that do not dissolve into a liquid solvent such as oil and water

57
Q

To get mass of 1.11 mole of

c6h12o6g

A

Add up atomic masses of each element and times by 1.11

58
Q

Calculating osmolality

A

1 kg per SOLVENT

59
Q

Calculating molarity

A

I liter SOLUTION

60
Q

Calculating molality

A

1 kg SOLVENT

61
Q

Tonicity

A

Comparing two solutions in terms of hypotonic (decrease osmolartity) isotonic (no change)
Hypertonic (increase osmolarity)

62
Q

Hypotonic

A

Decrease osmolarity

63
Q

Hypertonic

A

Increase osmolarity

64
Q

Isotonic

A

No change

65
Q

Normal osmolarity

A

270-290

66
Q

Normal saline

A

.09%

67
Q

Arrhenius theory

A

Acids in water dissociate and produce hydrogen ions (H+), bases in water dissociate and produce hydroxide ions (OH-)

68
Q

Lowry bronstead theory

A

The molarity of hydronium ion or hydroxide ion in pure water is 1x 10(-7) moles/liter

69
Q

Amphoteric

A

Will accept and donate a proton

70
Q

A polar solvent when placed in aqueous solution…

A

Separate in two particles, a cation (+) and an anion (-) at the ionic bond.

71
Q

1 mM= ? Meq

A

1mM=1mEq

Salts, 1mM=2 mEq

72
Q

Carbon can blank and blank

A

Receive and donate electrons

73
Q

Two types of isomers

A

Structural and stereo

74
Q

Carbon always has how many bonds

A

Four

75
Q

g=mL

A

L=kg

76
Q

Octect rule doesn’t apply to

A

Helium and hydrogen

77
Q

Meters to cm

A

Move decimal 2 points to right

78
Q

Benzene doesn’t have 4 bonds or

A

4 other atoms

79
Q

Lowery bronstead

A

Pure water equal # of hydronium and hydroxide

80
Q

1 mM potassium chloride =

1 mM calcium chloride =

A

1 mEq

2 mEq

81
Q

Ammonia and water

A

Increase OH-, decrease H30+ and increase pH

82
Q

Alkanes

A

Saturated with hydrogen

83
Q

Alkenes

A

Are not saturated with hydrogen

84
Q

Alkynes

A

Triple bonds and not saturated

85
Q

Aromatic rings

A

Contains six carbons in a ring, have a sweet smell

86
Q

Polarized light when passed through L amino

D-gycose?

A

Will
Rotate to the left

To the right

Chemistry (5 decks)

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