CHEM 101 Prelims

Chemistry

referred to as the central science

Reagents

substance or mixture for use in chemical analysis or other reactions

Clean, dry spatula

used in getting solds out of reagent bottlle

Organic solvents

are solvents immiscible with water

Material Safety Data Sheet

document that provides workers with procedures for safety handling or working

Beaker

reaction container, used to catch liquids from titrations

Bunsen Burner

sources of heat

Burets

for addition of a precise volume of liquid

Clay Triangles

placed on a ring attachment as support

Droppers

addition of liquids drop-by-drop

Erlenmeyer Flasks

hold samples and reactions, catch filtrates

Glass Funnels

funelling liquids and equipped with filter paper

Graduated Cylinders

measurement for liquid, nearest 0.1 mL

Hot Plates

source of heat when an open flame is not desirable

Pipets

dispense small quantities of liquid

Ring stand with Ringss

holding pieces of glassware in place

Test Tubes

holding small samples

Test tube holders

for holding test tubes

Volumetric Flasks

measure precise volumes or to make precise dilutions

Dilutions

solid dissolved to liquid chemical

Wash bottles

dispensing small quantities of distilled water

Watch glasses

holding small samples

Wire Gauze

supports beakers to be heated by Bunsen burners

Balances

determine the mass of a reagent or object

Spectrophotometers

measure the absorbance of transmittance of a liquid sample

Fume hoods

ventilate noxious or harmful gases

Meniscus

curve at the surface of a liquid

Hypothesis

tentative explanation of observations that acts as a guide

Scientific theories

well-substantiated explanations of particular aspects of nature

Scientific method

path of discovery from questions to hypothesis combined with verification

Qualitative Observation

also called a measurement, has number and a scale

Standard unit of Mass

kilogram

Standard unit of Length

meter

Standard unit of Time

second

Standard unit of Temperature

kelvin

Standard unit of Electric Current

ampere

Standard unit of Amount of Substance

mole

Standard unit of Luminous Intensity

candela

Exponential notation and symbol for prefix kilo-

$10^3$ ($k$)

Exponential notation and symbol for prefix deci-

$10^{-1}$ ($d$)

Exponential notation and symbol for prefix centi-

$10^{-2}$ ($c$)

Exponential notation and symbol for prefix milli-

$10^{-3}$ ($m$)

Exponential notation and symbol for prefix micro-

$10^{-6}$ ($\mu$)

Exponential notation and symbol for prefix nano-

$10^{-9}$ ($n$)

Exponential notation and symbol for prefix pico-

$10^{-12}$ ($p$)

Exponential notation and symbol for prefix femto-

$10^{-15}$ ($f$)

Exponential notation and symbol for prefix giga-

10⁹ (G)

Exponential notation and symbol for prefix mega-

10⁶ (M)

Fundamental Quantities

measured by the direct method

Derived Quantities

combination of fundamental quantities

Accuracy

agreement of a particular value

Precision

degree of agreement among several measurements

Unit factor method or Dimensional Analysis

convert a given result from one system of units to another

Conversion factor: liter to cubic meter

1L=10^-3m³

Conversion factor: inch to centimeter

1in=2.54cm

Conversion factor: kilogram to pounds

1kg=2.205lb

Conversion factor: pound to ounces

1 lb=16 oz1lb=16oz

Freezing point of F

32F

Boiling point of F

212F

Freezing point of C

0C

Boiling point of C

100C

Conversion: F to C

F = (1.80 x C) + 32

Conversion: C to F

(F - 32) / 1.80

Conversion: C to K

K = C + 273.15

Matter

defined as anything that occupies space and has mass

Three states of Matter

Solid, Liquid, Gas

Solid

rigid and possesses a definite shape

Liquid

flows and takes the shape of its container

Gas

takes both shape and volume of its container

Plasma

gaseous matter that contains electrically charged particles

Mass

measure of the amount of matter

Weight

force that gravity exerts

Law of Conservation of Matter

no detectable change in the total quantity of matter present when matter converts

Atom

smallest particle of an element

Indivisble

meaning of the Greek word atomos

Pure substance

has constant composition

Element

made of only one type of atom

Compound

two or more different atoms bonded together

Mixture

two or more different substances that are not chemically joined

Homogenous

mixture you cannot see the different parts

Heterogenous

you can see the different parts

Physical Property

characteristic of matter that is not associated with a change in its chemical composition

Physical change

change in the state without change in its chemical composition

Density, color, hardness, melting and boiling points, electrical conductivity

examples of physical properties

wax melting, sugar dissolving, steam condenses into liquid water

examples of physical change

Chemical Property

includes flammability, toxicity, acidity, reactivity, and heat combustion

Extensive property

property depends on the amount of matter present

Intensive Property

sample of matter does not depend on the amount of matter present

Chemical reaction

process in which a substance is changed into one or more new substances

Reactants

starting materials in a chemical reaction

Product

substance formed as a result of a chemical reaction

Combustion Reactions, A + B → AB

two or more substances combine to form one product

Decomposition Reaction AB → (with heat) A + B

compound decomposed to form two or more substances

Displacement Reaction, AY + B → BY + A

more active metal can displace a less active metal, refers to the activity series

Electromotive or activity series

arranged in the order of decreasing activity

Metathesis or Double Displacement Reaction, AX + BY → AY +BX

positive ions exchange partners with the negative ions to form two new compounds

Neutralization

result is salt

Combustion Reaction

reaction of elements and compounds with oxygen

Stoichiometry

describe quantitative relationships in Chemistry

Moles

used to calculate the amount of product formed in a reaction