Chemistry - Final Exam (Chapters 1, 2, 3, 4, 5)

ch 1. measurements have two parts: a \___ and a \___

number, scale

ch 1. the scale is called a \___

unit

ch 1. what are the two major systems of measurements?

English system and metric system

ch 1. what is the modified metric system called?

the international system of units/system international (SI unit)

ch 1. SI unit of mass

kilogram (kg)

ch 1. SI unit of length

meter (m)

ch 1. SI unit of time

second (s)

ch 1. SI unit of temperature

Kelvin (K)

ch 1. SI unit of electric current

ampere, A

ch 1. SI unit of amount of substance

mole (mol)

ch 1. SI unit of luminous intensity

candela (cd)

ch 1. derived units

Units we get from the base units

ch 1. derived unit of area

square meter (m^2)

ch 1. derived unit of volume

cubic meter (m^3)

ch 1. derived unit of force

Newton (N)

ch 1. derived unit of pressure

Pascal (Pa)

ch 1. derived unit of energy

Joule (J)

ch 1. derived unit of voltage

Volt (V)

ch 1. derived unit of frequency

Hertz (Hz)

ch 1. derived unit of electric charge

Coulomb (C)

ch 1. mega- (M)

10^6 (1,000,000)

ch 1. Kilo- (K)

10^3 (1,000)

ch 1. deci- (d)

10^-1 (0.1)

ch 1. centi- (c)

10^-2 (0.01)

ch 1. milli- (m)

10^-3 (0.001)

ch 1. micro- (μ)

10^-6 (0.000001)

ch 1. nano- (n)

10^-9 (0.000000001)

ch 1. pico- (p)

10^-12 (0.000000000001)

ch 1. why are measurements always uncertain?

* instruments have their flaws
* Measuring always involve estimation
* All measurements have certain or exact digits, uncertain or estimated digits

Symbol for uncertainty in measurement is…

±

ch 1. leading zeros

never significant ex) 0.00012 = 2 significant figures

ch 1. captive zeros

always significant ex) 2.003 = 4 significant figures

ch 1. trailing zeros

only significant if there is a decimal ex) 600 = 1 significant figures

ch 1. nonzero integers

always significant ex) 3453 = 4 significant figures

ch 1. Rules for Multiplication and Division of Significant Figures

leave your answer in the same number of significant figures as the number with the least significant figures ex) 4.36 x 1.2 = 5.232, Answer = 5.2

ch 1. Rules for Addition and Subtraction of Significant Figures

Leave your answer in the same number of decimal places as the measurement with the least decimal places ex) 12.11 + 18.0 + 1.013 = 31.123 Answer = 31.1 (because 18.0 has 1 decimal place)

ch 1. density equation

D=M/V

ch 1. volume equation

V=M/D

ch 1. mass equation

M=DV

ch 1. what are the two factors to determine reliability in measurement?

precision and accuracy

ch 1. precision

Degree of agreement among many measurements of the same quality

ch 1. accuracy

How close a measurement is to the accepted value

ch 1. scientific notation

short way of writing a very large number or measurement

ch 1. percentage error

% error = value accepted-value expected/value accepted x 100

ch 1. dependent variable

a variable whose value depends on that of another

ch 1. independent variable

a variable whose value doesn't depends on that of another

ch 1. pure substance

a pure substance is one with a fixed or constant composition

ch 1. elements

a pure substance made of one kind of atom & cannot be broken down into a simpler substance by any chemical or physical process

ch 1. compound

made up of two or more different elements or atoms chemically bonded together

A Pure Substance with a fixed composition

ch 1. mixtures

a blend of two or more substances that aren't chemically bonded

ch 1. homogeneous mixtures

you cannot see the different parts of the mixture

ch 1. heterogeneous mixtures

you can see the different parts of the mixture

ch 1. methods for separating mixtures

Filtration (Ex. The Sand & Filter Paper)

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Evaporation (Ex. The Salt In The Water Lab)

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Distillation (Differences in Boiling Points)

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Crystallization (the impure substance is dissolved in water, then filtered, then heated slowly, then cooled slowly leaving pure crystals formed without impurities)

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Chromatography (Composition Moves @ Different Paces)

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Magnetization ( Magnetic Material vs Non-Magnetic Material ) Ex. Iron & Magnet

Ddecantation ( Liquid vs. Solid ) Ex. Pasta & Water

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Electrolysis - CHEMICAL PROCESS (Ex. Hydrogen Atoms from Oxygen Atoms in Water)

ch 1. types of energy

mechanical energy, potential energy, kinetic energy

ch 2. physical property

observable characteristics of matter in which no new matter is formed

ch 2. chemical property

observable characteristics of matter in which a new substance is always formed

ch 2. physical change

no new matter is formed

ch 2. chemical change

new matter is always formed

ch 2. what are some evidences of a chemical change?

* formation of gas or bubble


* changes in temp.
* formation of precipitate
* color change

ch 2. what are the states of matter?

gas, liquid, solid, plasma

ch 2. conduction

the transfer of thermal energy by the collision of particles when objects or substances are in contact

ch 2. convection

process by which heat is transferred by movement of a heated fluid such as air or water

ch 2. radiation

a mode of energy transfer that occurs when thermal energy is transferred through waves

ch 2. open system

matter and energy can flow into or out of the system through its boundaries

ch 2. isolated system

matter and energy do not flow into or out of an isolated system

ch 2. closed system

energy may cross the system boundaries but matter cannot

ch 3. who discovered the electron?

JJ Thomson

ch 3. who discovered the proton?

Ernest Rutherford

ch 3. who discovered the neutron?

James Chadwick

ch 3. who created the Law of Conservation of Matter/Mass?

Antonine Lavoisier

ch 3. Law of Conservation of Matter/Mass

states that matter cannot be created nor destroyed

ch 3. who created the Law of Constant Composition?

Joseph Proust

ch 3. Law of Constant Composition

states that a given compound always has the same elements in the same proportions

ch 3. Dalton's Atomic Theory

* each element is made up of tiny particles called atoms
* atoms of a given element are identical
* chemical compounds are formed when atoms of different elements combine with each other

ch 3. JJ Thomson's model of atom

concluded that atoms have negatively charged particles or electrons. But atoms are electrically neutral. Meaning they must have equal negative and positive charges

ch 3. Rutherford's model of the atom

concluded that an atom's positive charge and most of its mass are in the center of the atom called the nucleus with negatively charged electrons moving around the nucleus and its empty space

ch 3. Bohr's model of the atom

atom is a small positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus

ch 3. Modern Atomic Theory

an atom contains protons, neutrons, and electrons

ch 3. the charge of a proton

positive

ch 3. the charge of a neutron

no charge

ch 3. the charge of an electron

negative

ch 3. location of a neutron

in the nucleus

ch 3. location of an electron

outside of the nucleus

ch 3. location of a proton

in the nucleus

ch 3. atomic number

the number of protons in an atom

ch 3. mass number

the sum of protons and neutrons in an atom or protons and neutrons (has no decimals)

ch 3. atomic mass/weight

the average mass of the relative abundance of the isotopes of an element (has decimals as seen in the periodic table)

ch 3. isotopes

atoms with the same number of protons but different numbers of neutrons

ch 3. atom's charge when it loses electrons

positive

ch 3. atom's charge when it gains electrons

negative

ch 3. where is mass number labelled on an ion?

top left

ch 3. where is atomic number labelled on an ion?

bottom left

ch 3. where is the electron and its charge labelled on an ion?

top right

ch 4. amplitude

height of wave measured from origin to crest, or peak

ch 4. wavelength

distance between successive crests of wave; distance that wave travels

ch 4. frequency

tells how fast the wave oscillates up and down

ch 4. hertz (Hz)

cycle per second

ch 4. speed of light

light moves through space at 3.00 x 108 meters per second

ch 4. visible spectrum

array of colors

ch 4. wavelength formula

λ = c / v (wavelength = speed of light / frequency)