Chemistry Test 1

Boiling point of Kelvin

373 K

Robert Millikan

used the Oil drop experiment to find the charge and mass of an electron

the mole is know as

Avogadro's number

blackbody radiation

the light given off by the heat of an object

p subshell

l=1, 3 orbitals

Systemic error

always high or low

nano scientific notation

10^-9

micro scientific notation

10^-6

solids

there is a set shape and set volume (think pressure)

Celsius to Fahrenheit

F= 9/5 (C+32)

compound

a substance composed of two or more elements in fixed defined proportions

example of a compound

water

Law of Multiple Proportions

when two elements (a,b) form two different compounds, the mass of the element "b" that combine with 1g of element "A" in reach substance can be expressed as a ratio of small whole numbers

symbol for fluorine

F

Symbol for Neon

Ne

anion

atom gains an electron and becomes (-) charged

visible light

a type of electromagnetic radiation and energy embodied by the oscillation of an electric and magnetic field

amplitude

Height of a wave

Subatomic Particles: If an atom has different numbers of protons and electrons, it will be

charged

the larger the shell number

the larger the orbital

Measurement

a comparison against an exact invariable standard unit

analog instrument

shows divisions

example of analog instrument

meter stick and graduated cylinder

Digital instrument

gives numerical read out

Example of Digital instrument

digital balance and digital thermometer

Accuracy

how close to the true valve you are

Random error

sometimes high, sometimes low

significant figures

collectively all the certain digits and the first uncertain

All _______ digits are significant

nonzero

_________ are not significant

leading zeros

___________ are always significant

sandwich zeros

_________________ are only significant after a decimal place

trailing zeros

Raw Answer

Answer after calculation that doesn't worry about sig-figs

when you add or subtract, the answer must end in the _________ decimal place common

lowest

Kilo scientific notation

10^3

Deci scientific notation

10^-1

Centi scientific notation

10^-2

1 kg= ____g

1000 g

1 g= ___cg

100

1 g= ___ micro grams

1,000,000 micrograms

1 g= ___ dg

10

1 g= ___ mg

1000 mg

1 g= ____ ng

1,000,000,000 ng

Exact Number

has infinite numbers of sig-figs and must be defined/fixed

example of exact number:

100 cm in a meter

Chemisrty

study of matter

what 5 things do we study about matter?

composition, structure, states, changes, and energy

What is matter?

stuff... anything that has mass and volume

particulate

composed of particles

composition and structure determine...

function

atom

smallest particle of matter to have both unique chemical and physical properties

molecules

made up of atoms binding together

state

depends on the relative position of the particles... due to strength of interactions and temperature

liquids

there is only a set volume (think less pressure/ tiny energy)

gas

there is no set volume and no set shape (think high energy)

composition

a listing of the types of atoms present as well as amounts

structure

how those atoms are connected and the order they are in

physical change

change in appearance without change in composition

physical property

anything you can say/do to a substance and maintain composition

chemical change (reaction)

change in composition so the ratio of atoms changes so you end up with something different from what you started with

engery

the ability to do work

potential energy

stored energy due to position

kinetic energy

energy possessed by moving

Temperature

A measure of how hot or cold something is.

freezing point at Fahrenheit

32 degrees

Boiling point at Fahrenheit

212 degrees

freezing point at Celsius

0 degrees

Boiling point at Celsius

100 degrees

freezing point at Kelvin

273 K

Fahrenheit to Celsius

C=5/9(F-32)

Celsius to Kelvin

K=C+273

Kelvin to Celsius

C=K-273

pure substance

made up of only one type of atom that has a fixed composition and does not vary

element

substance that cannot be chemical broken down into anything smaller

Example of an element

helium

molecules

combinations of two or more atoms bonded together

mixture

a substance composed of two or more types of atoms in proportions that can vary

hetergoneous mixture

ones in which the composition varies from one region to another inside

Example of a Hetergeneous Mixture

chocolate chip cookie or beach sand

homogeneous mixture

ones in which the composition is consistent

example of homogeneous mixture

Hershey's syrup and tea

who proposed the atom?

Democritus and Leucippus

Law of Conservation of Mass

the matter is neither created nor destroyed in a normal chemistry reaction

chemical reaction

a process in which one or more substances are converted into one or more different substances

each element is composed of tiny _____________ atoms

indestructible

all atoms of the same element have the same ________ and other _________ that make them different from other atoms of other elements

mass, properties

atoms of different elements combine in simple, ___________ ___________ ________ to form compounds

whole number ratios

JJ Thomson

discovered the electron

Plum Pudding Model

J.J Thomson's model of an atom, in which he thought electrons were randomly distributed within a positively charged cloud

Ernest Rutherford

used the Gold foil experiment to discover the nucleus

Nucleus

Center of an atom

Proton

positively charged particle

Chadwick

Discovered the neutron

Symbol for Hydrogen

H

Symbol for Helium

He

Symbol for Lithium

Li

Symbol for Beryllium

Be

Symbol for Boron

B

Symbol for Carbon

Ca

Symbol for Nitrogen

N