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KLowe Chemistry And Physics Larmon > Lecture 5: Chemistry Review > Flashcards

Lecture 5: Chemistry Review Flashcards

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1
Q

Atomic number (Z)

A

Number of protons, determines the identity of the atom

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2
Q

What are ions?

A

Atoms/groups of atoms bonded together with a net charge

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3
Q

Two types of ions

A
  • Cations

- Anions

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4
Q

Cation

A

Positively charged ion

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5
Q

Anion

A

Negatively charged ion

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6
Q

Elements contain…

A

Only 1 type of atom

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7
Q

Compounds contain…

A

More than one kind of atom in a fixed ratio by mass

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8
Q

What are molecules?

A

Groups of atoms chemically bonded together into a discrete unit by covalent bonds; neutral charge

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9
Q

What are ionic compounds?

A
  • Contain both positively and negatively charged ions with no identifiable units
  • Attracted by charge and are not molecules
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10
Q

Can a substance be both a molecule and an element?

A

Yes

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11
Q

What is a physical change?

A

No change in the chemical makeup (i.e.: melting ice)

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12
Q

What is a chemical change?

A

Always makes a chemically different substance (i.e.: 2H2O —> 2H2 + O2)

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13
Q

What is a physical property?

A

May be observed/measured without changing the chemical makeup

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14
Q

What are two types of physical properties?

A
  • Intensive

- Extensive

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15
Q

What is an intensive physical property?

A

Integral to the material, regardless of amount (i.e.: color)

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16
Q

What is an extensive physical property?

A

-Depends on sample size (i.e.: volume)

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17
Q

What is a chemical property?

A

Describes the type of chemical changes the material tends to undergo (i.e.: flammable)

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18
Q

Boiling water to steam

A

Chemical property

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19
Q

Liquid

A

Intensive physical property

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20
Q

Mass

A

Extensive physical property

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21
Q

What are substances?

A

Pure materials that can’t be physically separated into simpler components; can be compounds or elements

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22
Q

Throughout all samples, the chemical and physical properties of substances are ___

A

Uniform

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23
Q

What is a mixture?

A

2 or more pure substances

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24
Q

Physical processes can separate the mixture into ___

A

Simpler substances

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25
Q

Two types of mixtures

A
  • Homogeneous

- Heterogeneous

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26
Q

What is a homogeneous mixture?

A

Uniform in physical and chemical properties throughout the whole sample (i.e.: normal saline)

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27
Q

What is a heterogeneous mixture?

A

Distinct phase boundaries where chemical and/or physical properties change (i.e.: emesis)

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28
Q

Protons and neutrons are in the ___

A

Nucleus

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29
Q

Electrons are located ___

A

Around the nucleus in cloud-like orbitals

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30
Q

Atoms have ___ properties rather than geometric properties

A

Wave-like

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31
Q

All atoms have ___ and ___

A

Protons and electrons

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32
Q

All atoms contain ___ except for ___

A

Neutrons except for hydrogen

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33
Q

Atomic Number (Z) =

A

Number of protons, determines identity

Ex: Carbon Z = 6

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34
Q

Neutron number (N) =

A

Number of neutrons

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35
Q

Mass number (A) =

A

Z + N

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36
Q

Atomic mass is measured in ___

A

Amu

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37
Q

Protons and neutrons are ~ ___ amu

A

~1 amu; leads to mass deficit

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38
Q

The mass number can never be smaller than…

A

The atomic number

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39
Q

What are isotopes?

A

Same atomic number, different mass number (diff number of neutrons, same number of protons)

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40
Q

Dalton’s Atomic Theory—Elements are composed of tiny, indivisible particles called ___. All atoms of a given element are…

A

Atoms; identical and unique to that element

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41
Q

Dalton’s Atomic Theory—Compounds are formed by…

A

Bonding atoms together in a fixed ratio

42
Q

Dalton’s Atomic Theory—Chemical reactions do not ___, ___, or ___ … Chemical reactions cause atoms to…

A

Create, destroy, or change atoms into atoms of other elements; recombine into new substances

43
Q

What is the Law of Conservation of Mass?

A
  • No detectable change in the total mass occurs during a chemical reaction
  • The components are neither created, nor destroyed—they recombine
44
Q

What is the Law of Definite Proportions?

A

Different samples of a pure compound always contain the same elements in the same proportion by mass

Ex: Water = 11.2% hydrogen and 88.8% oxygen by mass

45
Q

What is the Law of Multiple Proportions?

A

Some elements can combine to give more than one compound

Ex: Carbon burned in oxygen produces both carbon dioxide and carbon monoxide

46
Q

What is the Periodic Law?

A

Properties of elements are periodic functions of their atomic numbers

47
Q

The periodic table is arranged in order of…

A

Increasing atomic number

48
Q

Vertical on the periodic table

A

Groups/families; similar chemical and physical properties

49
Q

Rows on the periodic table

A

Periods

-Adding electrons to energy levels, electron shells

50
Q

The element at the end of the row has the outer shell ___

A

Full of electrons

51
Q

Elements with nearly full electron shells ___

A

Accept electrons

AKA anions

52
Q

Elements with nearly empty electron shells readily ___

A

Release electrons

AKA cations

53
Q

The atomic weights listed on the periodic table are ___

A

An average of all isotopes—no element is the exact weight listed

54
Q

Representative elements are located…

A

In the high rises on the left and right

55
Q

Transition elements are located between ___

A

the representative elements

56
Q

Inner transition elements are located…

A

At the bottom of the table

57
Q

Most elements are ___ and are on the ___ side of the table

A

Metals, left side

58
Q

Properties of metals (5)

A
  • Shiny luster
  • Ductile
  • Malleable
  • Good conductors of heat and electricity
  • React to form cations by giving away electrons
59
Q

Ductile =

A

can stretch out; can stretch it out into a thin wire

60
Q

Malleable =

A

Can pound it into submission; change its shape

61
Q

Non-metals are located on the ___ side of the table

A

Right

62
Q

Properties of non-metals (4)

A
  • Liquids, solids, or gases
  • Solids tend to be brittle
  • Do not conduct
  • Tend to form anions
63
Q

Metalloids are located along ___

A

The ladder

64
Q

Properties of metalloids (4)

A
  • Intermediates
  • Shiny luster
  • Less malleable and ductile than metals
  • Conduct electricity but not well—semiconductors
65
Q

Most elements are ___

A

Solids

66
Q

Mercury and bromine are ___

A

Liquids

67
Q

Gallium will ___

A

Melt in your hand

68
Q

Hydrogen, nitrogen, oxygen, fluorine, chlorine, and all noble gases are ___

A

Gases

69
Q

What is electricity?

A

The flow of charged particles under the influence of an electric field

70
Q

What is an electrolyte?

A

A substance that dissolves in water to give a solution conductivity

71
Q

Most molecular compounds are considered ___

A

Non-electrolytes

72
Q

Why does dissolution of electrolytes occur?

A

Because water interacts very effectively with ions

73
Q

Water itself is a ___

A

Non-electrolyte

74
Q

Aluminum (Al)

A
  • Silvery white metal
  • Low density
  • Does not occur naturally in nature, must be synthesized
  • Found in antiperspirants (aluminum chloride) and antacids (aluminum hydroxide)
75
Q

Aluminum should be avoided in ___ patients

A

Dialysis patients—can build up and be toxic

76
Q

Barium (Ba)

A
  • Used in radiographic GI studies—barium sulfate oral solution or enemas
  • Heavy metal, relatively opaque to x-rays
  • Toxic, but patients will excrete the material fairly easily
77
Q

Bromium (Br)

A
  • One of 2 naturally occurring liquids

- Highly toxic

78
Q

Calcium (Ca)

A
  • Silvery white
  • Doesn’t occur naturally in nature in the elemental form
  • Muscle contraction, bone stability
  • Found in antacids, phosphate binders
79
Q

Carbon (C)

A
  • Graphite and diamond occur naturally
  • Activated charcoal—used in overdoses
  • In most compounds, highly versatile
80
Q

Chlorine (Cl)

A
  • Toxic green gas
  • Disinfectant
  • Clorox, other cleaners
81
Q

Chromium (Cr)

A
  • Silvery white metal
  • Forms highly colored compounds
  • Found in stainless steel
82
Q

Copper (Cu)

A
  • Reddish metal

- Great conductor

83
Q

Fluorine (F)

A
  • Yellow, poisonous gas

- Sodium fluoride strengthens teeth

84
Q

Helium (He)

A
  • Colorless, inert gas

- MRI coolant

85
Q

Hydrogen (H)

A
  • Most common atom in the universe (> 95% of all known matter)
  • Colorless, flammable gas
86
Q

Iodine (I)

A
  • Purplish/black solid

- Found in topical antiseptics and anti thyroid medications

87
Q

Iron (Fe)

A
  • Found in each hemoglobin molecule to transport oxygen through the blood
  • Metal
88
Q

Lithium (Li)

A
  • Silvery, highly reactive metal

- Used as a mood stabilizer for bipolar patients

89
Q

Magnesium (Mg)

A
  • Silvery white metal
  • Important for cardiac conduction and potassium levels
  • Tocolytic therapy
  • Laxative
90
Q

Nitrogen (Ni)

A
  • Colorless, odorless gas
  • 80% of air
  • Found in anesthetic gas as nitrous oxide (N2O)
91
Q

Oxygen (O)

A
  • Odorless, colorless, reactive gas

- Strong tendency to accept electrons, important in ATP synthesis

92
Q

Phosphorus (P)

A
  • Found in RNA and DNA and in ATP
  • Low phosphorus may cause brittle bones and respiratory failure
  • Supplemented in salt forms with sodium or potassium
93
Q

Potassium (K)

A
  • Silvery white metal, highly reactive
  • Important for muscle contraction
  • Inverse relationship with insulin
  • Electrolyte—affected by ACE inhibitors, loop diuretics
94
Q

Sodium (Na)

A
  • Muscle contractions

- CNS stability, water balance

95
Q

Titanium (Ti)

A
  • Grayish metal

- Found in prosthetic implants—lightweight, low toxicity, high strength

96
Q

Zinc (Zn)

A
  • Bluish silver metal

- Calamine lotion, sunblock, wound healing, cold symptom relief

97
Q

Molecular compounds are comprised only of ___

A

Nonmetals

98
Q

Ionic compounds are almost always comprised of ___

A

A metal and a nonmetal

99
Q

What are ionic compounds?

A

Sometimes referred to as salts—reaction of an acid with a base

100
Q

What are polyatomic ions?

A

Formed when 2 or more nonmetal atoms are bonded together in a way that results in a net electrical charge

KLowe Chemistry And Physics Larmon (11 decks)

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