Chapter 2.2 Flashcards

1
Q

Matter

A

anything that has weight and takes up space. This includes all solids, liquids, and gases in our surroundings as well as in our bodies

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2
Q

Atom

A

smallest particle of an element that has properties of that element

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3
Q

Elements

A

The simpliest examples of matter with specific chemical properties

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4
Q

COmpounds

A

Some elements exist in a pure form, but these and other elements are more commonly parts of chemical combinations

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5
Q

Bulk elements

A

elements the body requires in large amount - carbon, hydrogen, oxygen, nitrogen, sulfur

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6
Q

Trace Elements

A

Elements required in small amounts

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7
Q

Ultratrace elements

A

some elements that are toxic in large amounts, but may be vital in very small amounts

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8
Q

Chemical Bonds

A

Some atoms can combine with atoms like themselves or with other atoms by forming attractions

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9
Q

Nucleus

A

A central portion of an atom

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10
Q

Electrons

A

One or more that constantly move around the nucleus

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11
Q

Protons/Neutrons

A

Are equal in weight but have different electrical properties.

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12
Q

Atomic Number

A

The number of protons in the atoms of an element

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13
Q

Atomic Weight

A

The number of protons plus the number of neurtons in each of an elements atoms

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14
Q

Isotopes

A

Atoms that have same atomic number but different atomic weights.

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15
Q

Three common forms of atomic radiation

A

Alpha, Beta, and Gamma

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16
Q

Beta radiation consists..

A

of much smaller particles that travel faster and more deeply penetrate

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17
Q

Alpha radiation consists

A

of particles from atomic nuclei , each of which includes two protons and neutrons

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18
Q

Gamma Rradiation consists of

A

a form of energy similar to x-radiation and is most penetrating form of atomic radiation

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19
Q

Molecules

A

Two or more atoms may combine to form a distinctive type of particle

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20
Q

Molecular Formula

A

Shorthand used to depict the numebr and types of atoms in a molecule.

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21
Q

Bonds

A

Atoms combining with other aroms by forming links. Chemical bonds result from interaction of electrons.

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22
Q

Octet Rule

A

Atoms react in a way that leaves the outermost shell completely filled with electrons, achieving a more stable structure

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23
Q

Inert

A

When the outermost electron shells are filled, already have stable structures and are chemicall inactive

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24
Q

Ions

A

Atoms that gain or lose electrons become electrically charged

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25
Cations
Postively charged ions
26
Anions
negatively charged ions
27
Ionic Bonds
Ions with opposite charges attract
28
Covalent Bond
A chemical bond between aotoms that share electrons
29
Polar Bond
Unlike an ion, a polar molecule has an equal number of protons and electrons but more of the electrons are at one end of the molecule making that end slightly negative while the other end of the molecule is slightly positive.
30
Hydrogen Bond
The attraction of the positive hydrogen end of a polar molecular to the negative nitrogen or oxygen end of another polar molecule
31
Synthesis
When two or more atoms, ions, or molecules bond to form a more complex sturcture as when hydrogen and oxygen atoms bond to form molecules of water, the reaction is called synthesis
32
Decomposition
If the bonds of a reactant molecule break to form simpler molecules, atoms or ions if the reaction
33
Exchange Reaction
Parts of two different types of molecules trade positions as bonds are broken and new bondsa re formed
34
Reversible Reaction
This means the product or products can be changed back to the reactant or reactants
35
Catalysts
Are molecules that influence the rates of chemical reactions but are not consumed in the process
36
Dissociate
When ionically bound substances are placed inw ater, the ions are attracted to the positive and negative ends of the water molecules and tend to leave each other or dissociate
37
Acids
Electrolyte that dissociate to release hydrogen ions inw ater
38
Bases
Substances that release ions that combine with hydrogen ions
39
Salts
Bases can react with acids to neutralize them, forming water and electrolytes
40
Acidic
Solutions with more hydrogen ions
41
Basic (Alkaline)
solutions with fewer hydrogen ions than hydroxide ions, pH values greater than 7
42
Alkalemia?
Blood pH of 7.5 to 7.8
43
Alkalosis?
Makes one feel agitated and dizzy.
44
Acidemia
Occurs when the blood pH falls to 7.0 to 7.3.
45
Acidosis
Makes one feel disoriented and fatigued, and breathing may become difficult.
46
Buffers
chemicals that resist pH change
47
Organic Compounds
have carbon and hydrogen
48
inorganic compounds
anything thats not organic
49
Electrolytes
Inorganic susbtances usually dissolve in water and dissociate forming ions
50
Nonelectrolytes
Most organic compounds that dissolve in water do not release ions
51
Solvent
A substance in which other susbtances dissolve. WAter is an important solvent
52
Solute
A substance dissolved ina solvent, such as water
53
Solution
The combination of a colvent and any solutes dissolved
54
Organelles use oxygen to
release energy from nutrient molecules
55
CO2
is a cimple carbon-containing inorganic compound. It is a waste product of the release of energy during certain metabolic reactions
56
Organic Substances
Important groups of chemical chemicals in cells including carbohydrates, lipids, proteins, and nucleic acids
57
Carbohydrates
Provide much of the energy that cells require. They also supply materials to build certain cell structures and they often are stored as reserve energy supplies. Water-soluble. Often have twice as many hydrogen as oxygen.
58
Simple carbohydrates are
sugars include monosaccharides and disaccharides
59
Monosaccharides may include
three to seven carbons in a straight chain or ring.
60
Disaccharides consist of
two simple sugar building blocks
61
Polyssaccharides
Complex carbohydrates. Built of simple carbohydrates linked to form larger molecules of different sizes. An example is cellulose.
62
Electrolyes
A solution that has electrically charged particles (ions), so it conducts an electric current. Substances that release ions in water are this
63
pH scale measures?
Hydrogen ion concentration