Chemical Principles Exam 1

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Modules 1-3. This set just contains Notes

35 Terms

1

Exponents on a Calculator

-e or e^x

example: -2 Ă— 10^5= 2e-5

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2

Log on a calculator

  • may need to enter number first then Log.

    • example log(100)=2

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3

Scientific Notation

  • cannot be greater than 10 nor less than one

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4

Order of Operations

PEMDAS

  • Parantheses

  • Exponents

  • Multiplication

  • Division

  • Addition

  • Subtraction

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5

Percentages

  • Percent (%) = /100

  • “of”= x (multiplication)

  • what= unknown quantity (x)

  • is = =(equals)

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6

Slope

rise/run

y2-y1/x2-x1

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7

chemistry

study of matter and energy

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8

matter

anything that has mass and takes up space

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9

elements

  • simplest form of matter

  • has distinct physical and chemical properties

    • building blocks of the universe

  • form attractions (Chemical bonds)

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10

Chemical Bonds

  • formed by atoms of different elements

  • can be broken and form new bonds with different atoms

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11

compound

chemical combination of elements that has its own set of properties and a chemical composition

  • pure water always contains the same two elements with the same proportions

    • 88.8% oxygen, 11,2% hydrogen by mass

  • Can only be separated through chemical reactions

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12

Chemical composition

the given ratio by mass of each element in a compound to any other element in the compound

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13

Elements and Compounds are defined as

Pure substances

  • A substance in which all of the particles that make up the substance are of exactly the same kind

  • two can physically combine to produce a mixture

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14

Mixture

not chemically bonded

  • can be separated by physical means

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15

in an element

atoms may be single or bound but all the same type

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16

in a compound

at least two different types of atoms bound together in a specific ratio

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in a mixture:

can be made of any combination of elements and and compounds and are not bonded to one another

not chemically bonded and be separated by physical means

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18

Heterogeneous

not uniform throughout

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19

homogeneous

uniform throughout

  • a solution

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20

Aqueous Solution

a solution in water

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21

Examples of Pure Substances

Elements & Compounds

  • hydrogen & sodium (element)

  • Table Salt Water (Compound)

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22

Examples of Mixtures

Heterogeneous and Homogeneous Mixtures

  • oil & water, chicken noodle soup (hetero)

  • brass and vodka (homo)

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23

Every substance has a definite set of

Properties

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24

Propeties

characteristics by which something can be identified

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25

Physical Properties

  • unrelated to changes in chemical composition

    • color, conductivity, & melting point

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26

Chemical Properties

Describes the characteristic ways that a substance can be identified

  • related to how it reacts chemically with another substance

    • reactivity

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27

Properties notes

chemists distinguish properties that are extensive or intensive

  • properties of compounds are constant and different from the elements there made of.

  • when matter undergoes change, the starting material is the reactant and the resulting material is the product.

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28

Extensive Properties

Depends of the Quantity

  • weight

<p>Depends of the Quantity</p><ul><li><p>weight</p></li></ul><p></p>
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Intensive Properties

remains unchanged regardless of the quantity

  • color

  • boiling point

<p>remains unchanged regardless of the quantity</p><ul><li><p>color </p></li><li><p>boiling point</p></li></ul><p></p>
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30

Physical Change

does not alter the chemical composition

  • boiling water changes the phase

  • separating a mixture into components ( a mixture of elements and compound)

    • might be separated into pure substances but the pure substances that result are the same ones that were in the mixture to begin with,

    • no pure substances were formed by separating a mixture into its components

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