Chemistry Chapter 1 And 2

Front 1

A value

Back 1

is a quantitative description that includes both a unit and a number.

Front 2

Units

Back 2

are quantities defined by standards that people agree to use to compare one event or object to another.

Front 3

length

Back 3

meter, m, the distance that light travels in a vacuum in 1/299,792,458 of a second

Front 4

mass

Back 4

kilogram, kg, the mass of a platinum-iridium alloy cylinder in a vault in France

Front 5

time

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second, s, the duration of 9,192,631,770 periods of the radiation emitted in a specified transition between energy levels of cesium-133

Front 6

temperature

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kelvin, K, 1/273.16 of the temperature difference between absolute zero and the triple point temperature of water

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1 L =

Back 7

10−3 m3

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103 L = 1 m3

Back 8

103 L = 1 m3

Front 9

Mass

Back 9

usually defined as a measure of the amount of matter in an object. Mass can be defined as the property of matter that leads to gravitational attractions between objects and therefore gives rise to weight.

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Matter

Back 10

is anything that occupies a volume and has a mass.

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weight

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of an object, on the Earth, is a measure of the force of gravitational attraction between the object and the Earth.

Front 12

Precision

Back 12

describes how closely a series of measurements of the same object resemble each other. The closer the measurements are to each other, the more precise the measurement. The precision of a measurement is not necessarily equal to its accuracy.

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Accuracy

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is a measurement’s relationship to the property’s true value.

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Accuracy can be defined as how close a number is to what it should be.

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Accuracy can be defined as how close a number is to what it should be.

Front 15

Chemistry

Back 15

The science that deals with the structure and behavior of matter

Front 16

model

Back 16

is a simplified approximation of reality

Front 17

Kinetic Molecular Theory

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All matter is composed of tiny particles.
The particles are in constant motion.
Increased temperature reflects increased motion of particles.
Solids, liquids and gases differ in the freedom of motion of their particles and in how strongly the particles attract each other.

Front 18

Solids

Back 18

Definite shape
Definite volume
Strong intermolecular or ionic forces.
Molecules (units) closely packed and in fixed positions.

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Liquids

Back 19

Constant volume but variable shape
The particles are moving fast enough to break the attractions between particles that form the walls of the cage that surround particles in the solid form.
Thus each particle in a liquid is constantly moving from one part of the liquid to another.

Front 20

Liquids

Back 20

Takes the shape of the container
Definite volume
Intermolecular forces weaker
Molecules are in close contact, however, there is freedom of movement (NOT fixed in place).

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Gas

Back 21

Variable shape and volume
Large average distances between particles
Little attraction between particles
Constant collisions between particles, leading to constant changes in direction and velocity

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Gas

Back 22

Completely fills the container
No definite volume
Weakest intermolecular forces
Sensitive to pressure
Molecules move about freely and maintain a relatively large average spacing.

Front 23

Metals have a shiny metallic luster.
Metals conduct heat well and conduct electric currents in the solid form.
Metals are malleable.
For example, gold, Au, can be hammered into very thin sheets without breaking.

Back 23

Metals have a shiny metallic luster.
Metals conduct heat well and conduct electric currents in the solid form.
Metals are malleable.
For example, gold, Au, can be hammered into very thin sheets without breaking.

Front 24

Atoms

Back 24

Tiny…about 10-10 m
If the atoms in your body were 1 in. in diameter, you’d bump your head on the moon.

Front 25

Particles in the Atom

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neutron, proton and electron

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Ions

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are charged particles due to a loss or gain of electrons.

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cations.

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When particles lose one or more electrons, leaving them with a positive overall charge.

Front 28

anions

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When particles gain one or more electrons, leaving them with a negative overall charge.

Front 29

cation

Back 29

ion with a positive charge
If a neutral atom loses one or more electrons
it becomes a cation.

Front 30

anion

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ion with a negative charge
If a neutral atom gains one or more electrons
it becomes an anion.

Front 31

Isotopes

Back 31

are atoms with the same atomic number but different mass numbers.

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Isotopes

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are atoms with the same number of protons and electrons in the uncharged atom but different numbers of neutrons.

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Isotopes

Back 33

are atoms of the same element with different masses.

Front 34

Atomic Mass Units, u, (or amu) :

Back 34

a mass unit which gives the mass of a particle relative to the carbon 12 isotope

Front 35

Atomic Number

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the number of protons in the nucleus. The identity of an element is due to the number of protons in the nucleus. In a (neutral) atom the number of protons and the number of electrons are equal!

Front 36

Ion

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if an atom gains or loses electrons it will posses a net electric charge and is then known as an ion.

Front 37

positive ion- cation negative ion –
anion

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positive ion - cation negative ion – anion

Front 38

Atomic Mass Number (A)

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The number of protons plus neutrons in the nucleus.

Front 39

Electrons

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Can be gained, lost, or shared…actively participate in chemical changes
Affect other atoms through their -1 charge

Front 40

Protons

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Affect other atoms through their +1 charge
Determine the number of electrons in uncharged atoms

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Neutrons

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No charge…no effect outside the atom and no direct effect on the number of electrons.

Front 42

Protons

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Affect other atoms through their +1 charge
Determine the number of electrons in uncharged atoms.

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base unit:

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The seven units from which all other units in the SI system of measurement are derived.

Front 44

precision:

Back 44

The closeness in value of a series of measurements of the same entity.

Front 45

accuracy:

Back 45

How closely a measured value approaches the true value of a property.

Front 46

Definition of value:

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A number and unit that together represent the result of a measurement or calculation, e.g. 100 meters.

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chemistry:

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The study of the structure and behavior of matter.

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Definition of model:

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A simplified approximation of reality.

Front 49

evaporation:

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The conversion of a liquid to a gas.

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Definition of element:

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A substance that cannot be chemically converted into simpler substances; a substance in which all of the atoms have the same number of protons and therefore the same chemical characteristics.

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Definition of metals:

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The elements that (1) have a metallic luster, (2) conduct heat and electric currents well, (3) are malleable, and (4) are solids at 20 °C (with the exception of the metal mercury, which remains a liquid at that temperature).

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Definition of nonmetals:

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The elements that do not have the characteristics of metals. Some of these are gases at room temperature and pressure, some are solids, and one is a liquid. They have various colors and textures.

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metalloids:

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The elements that have some but not all of the characteristics of metals.

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Definition of malleable:

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Capable of being extended or shaped by the blows of a hammer.

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atom:

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The smallest part of an element that retains the chemical characteristics of the element.

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Definition of proton:

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a positively charged particle found in the nucleus.

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Definition of electron:

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A negatively charged particle found outside the nucleus of an atom.

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An uncharged particle found in the nucleus of an atom.

Back 58

neutron

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Definition of nucleus:

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The extremely small, positively charged core of the atom.

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isotopes:

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Atoms that have the same number of protons but different numbers of neutrons. They have the same atomic number but different mass numbers.

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Definition of group:

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All the elements in a given column on the periodic table; also called a family.

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Definition of periods:

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The horizontal rows on the periodic table.

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atomic mass unit:

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Unit of measurement for the masses of particles; 1/12 the mass of a carbon atom that has 6 protons, 6 neutrons, and 6 electrons.

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The number of protons in an atom's nucleus. It establishes the element's identity.

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atomic number:

Front 65

The sum of the number of protons and neutrons in an atom's nucleus.

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Definition of mass number:

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ion:

Back 66

Any charged particle, whether positively or negatively charged.

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cation:

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An atom that has lost one or more electrons and thus has become positively charged.

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anion:

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An atom that has gained one or more electrons and thus has become negatively charged.

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covalent bond:

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A link between atoms that results from their sharing two electrons.

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diatomic:

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Composed of paired atoms.

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molecule:

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An uncharged collection of atoms held together with covalent bonds.

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representative elements:

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The elements in groups 1, 2, and 13 through 18 (the A-groups) on the periodic table; also called main-group elements.

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main-group elements:

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The elements in groups 1, 2, and 13 through 18 (the A-groups) on the periodic table; also called representative elements.

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transition metals:

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The elements in groups 3 through 12 (the B-groups) on the periodic table.

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inner transition metals:

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The 28 elements at the bottom of the periodic table.