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Chemistry > Chapter 1 & 2 > Flashcards

Chapter 1 & 2 Flashcards

1
Q

Atom

A

The smallest unit of an element that has the chemical properties of that element

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2
Q

Chemical formula

A

Describes the composition of a compound using the symbols for the elements that make up the compound

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3
Q

Compounds

A

Two or more elements combined in definite proportions

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4
Q

Elements

A

A substance that cannot be broken down into simpler substances even by chemical reaction

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5
Q

Heterogeneous mixture

A

A mixture that is not uniform throughout

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6
Q

Homogeneous mixture

A

Has a uniform mixture throughout often called a solution

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7
Q

Mass

A

A measure of the quantity of matter. The interaction of mass with gravity creates weight which is measured

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8
Q

Matter

A

Anything that occupies space and has mass

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9
Q

Liquid

A

Has no fixed shape, it takes the shape of the filled portion of It’s container, and it can be poured and can be compressed slightly.

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10
Q

Metals

A

Are distinguished by shiny luster and electrical conductivity

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11
Q

Gas

A

Has no fixed shape, it adopts the shape of its container expanding to fill the space completely and is easily compressed

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12
Q

Aqueous solution

A

A solution in which a substance is dissolved in water

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13
Q

Mixtures

A

A combination of two or more substances that can vary in composition

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14
Q

Physical properties

A

A characteristic that we can observe or measure without changing the composition of a substance

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15
Q

Pure substance

A

Matter that has the same chemical composition, no matter what its origin

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16
Q

Solution

A

A uniform or homogeneous mixture

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17
Q

Molecule

A

Two or more atoms bound together in a discrete arrangement

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18
Q

Physical state

A

A form that matter can take

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19
Q

Solid

A

Has a fixed shape that is not related to the shape of the container holding it and cannot be compressed

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20
Q

Volume

A

The amount of space a substance occupies

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21
Q

Density

A

The ratio of an objects mass to its volume

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22
Q

Temperature

A

The relative hot or cold something is to a standard

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23
Q

Kelvin

A

-273.15 degrees C

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24
Q

Physical change

A

Changing the physical properties of a substance without changing the chemical properties. Ex solid -> liquid -> gas

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25
Chemical changes
A process in which one or more substances are converted into one or more new substances
26
Chemical reaction
A chemical change in a substance
27
Chemical property
Is defined by what a substance is composed of and what chemical changes it can undergo
28
Energy
The capacity to do work or to transfer heat
29
Kinetic energy
The energy of motion
30
Potential energy
The energy possessed by an object because of its position
31
Work
Usually means mechanical work. When a force acts over distance.
32
Element symbol
Short hand version of an elements name
33
Scientific method
An approach to asking questions and seeking answers that employes a variety of tools, techniques and strategies 1. Obtain data, observations, or experiments 2. Recognize patterns or trends 3. Propose and test hypothesis -> 1 again 4. Propose theory -> 1 again
34
Hypothesis
A tentative explanation for the properties or behavior of matter that accounts for a set of observations and can be tested
35
Kinetic molecular theory
A model of ideal gas behavior; assumes that gas particles occupy no volume and that there are no intermolecular forces between them
36
Chemistry
The scientific study of matter and energy
37
Law of definite composition
=law of definite proportions = a specific compound always has a specific atom ratio and a specific percentage by mass of each element in the compound
38
Exothermic reaction
Heat energy is released during reactions
39
Endothermic reaction
Heat is taken in during reactions
40
Sublimation
Changing from a solid to a gas or from a gas to a solid without going through the liquid state
41
The law of conservation of mass
The mass of the products of a reaction always equals the mass of the reaction substances.
42
The law of definite proportions
All samples of the same compound always contain the same proportions by mass of the component elements
43
Subatomic particles
A smaller particle found inside an atom such as protons, neutrons, electons
44
Electron
Negatively charged subatomic particle
45
Proton
A positively charged subatomic particle
46
Neutron
An uncharged particle in the nucleus of an atom
47
Nucleus
The very dense region at center of an atom consisting of protons and neutrons
48
Atomic number
The number of protons in the nucleus of an atom
49
Isotope
An atom of an element that contains a specific amount of neutrons
50
Mass number
Of an isotope is the sum of the number of protons and the number of neutrons in its nucleus
51
Deuterium (D)
Hydrogen-2 often called "heavy water" it is used by chemists to observe specific hydrogen atoms in an experiment
52
Ion
When an atom contains more or less electrons
53
Cation
A positively charged ion. It contains less electrons than protons
54
Anion
A negatively charged ion. It contains more electrons than protons
55
Atomic mass unit (amu)
The basic unit of mass of atoms and molecules: | Exactly 1/12 the mass of Carbon -12
56
Relative atomic mass
The average of the mass of the individual isotopes, taking into account the naturally occurring relative abundance of each.
57
Metalloid
An element with physical properties like a metal but chemically reactivity more like that of a non metal
58
Main group element
Any element in one of the eight groups with the letter A
59
Transition metal /elements
An element in any of the 10 groups labeled with the letter B
60
Inner-transitional metal
Any element from the lanthanide or actinide group
61
Alkali metal
Any element in group IA except H(1) | Li, Na, K, Rb, Cs, Fr
62
Alkaline earth metals
Any element in group IIA(2) | Be, Mg, Ca, Sr, Ba, Ra
63
Halogen
Any element in group VIIA(17) | F, Cl, Br, I, At
64
Noble gas
Any element in group VIIIA(18) do not normally combine with other elements to form compounds He, Ne, Ar, Kr Xe Rn
65
Diatomic molecules
A molecule consisting of two atoms
66
Period
Are represented by Arabic numbers (1-7) in horizontal rows. Each period indicates amount of energy levels
67
Groups / families
These are represented by roman numerals (IA-VIIIA, representative elements and IB-VIIIB, transition elements) in verticals columns
68
The staircase
Separates the metals from the non-metals
69
Chemical nomenclature
System of names and formulas
70
Representative elements
IA-VIIA the A group or family
71
Dalton's Atomic Theory
1. All matter is composed of atoms 2. All atoms of a given element are identical both in mass and chemical properties 3. Atoms are not created or destroyed in chemical reactions 4. Atoms combine in simple, fixed, whole numbered ratios to form compounds
72
Thompson's model
Raisins (electrons) in plum pudding (sphere of positive charge)
73
Rutherford's model
Atom made up of positively charged nucleus surrounded by a cloud of orbiting electrons. Electrons release energy when while orbiting a nucleus so it would gradually spiral inwards, collapsing into the nucleus. SO all atoms would be unstable. (Planetary model)
74
Bohr's model
Electrons only travel in special orbits at certain discrete set of distances from the nucleus with specific energies. Electrons do not lose energy as they travel. They can only gain or lose energy by jumping form one allowed orbit to another

Chemistry (7 decks)

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