Chemistry Exam 1

gigameter

1 Billion Meters

kilometer

1 Thousand Meters

decimeter

1 Tenth of a Meter (0.1)

millimeter

1 Thousandth of a Meter (.0001)

centimeter

1 Hundredth of a Meter (.01)

micrometer

1 Millionth of a Meter (0.000001)

nanometer

1 Billionth of a Meter (0.000000001)

picometer

1 Trillionth of a Meter (0.000000000001)

What is the scientific unit for mass

Kilograms (1000 grams)

Scientific Unit for length

meters

scientific unit for temp

Kelvin (Celsius + 273.15)

Scientific Unit for time

seconds

what is density

mass/volume

What is Kelvin in terms of Celsius

Celsius + 273.15

I milligram = how many grams

0.001 grams

Cm³ = ?

1 mL

Precision

How close the measurements are to each other in a series

Accuracy

How close measurements are to actual value

systematic error

Measurements either being too high or too low

Random error

Measurements being both high and low

atomic number

number of protons in 1 atom

mass number

number of protons plus neutrons

Isotope

element with a different number of neutrons and therefor different mass number

element

the most basic kind of substance

atom

individual unit of an element (building block)

two or more atoms bounded together

molecule

pure substance

has properties that do not very between samples (i.e, element and compound)

mixture

physical combination of two or more pure substances; can be hetero or homogeneous

chemical combining of two or more pure substances

compound

do NOT rely on amount of material

intensive properties

examples of intensive properties

density color odor

DO rely on amount of material or substance

extensive properties

examples of extensive properties

mass volume

Dalton’s 1st Atomic Theory

Each element is composed of individual units called atoms

Dalton’s 2nd Atomic Theory

In a sample of a given element all atoms are identical

Dalton’s 3rd Atomic Theory

Two different elements will have different atoms

Dalton’s 4th Atomic Theory

Compounds are made by combining different elements. A given compound will always have the same type or ratio of atoms

Dalton’s 5th Atomic Theory

Atoms of 1 element cannot be changed into atoms of a different element. They can not be created or destroyed

Law of Constant Composition

in a chemical compound, the relative number of different atoms is constant throughout

Law of Mass Conservation

Total mass of substances present does not change during chemical reaction

Cathode Ray Tube Experiment

discovered that atoms have electrons, and that electrons have mass

Oil Drop Experiment

discovered the magnitude/measured an electrons charge, and was used to calculate the electrons mass

Rurtherford Gold Foil Experiment

discovered that the mass of an atom is in the nucleus in the center of the atom, and that an atom is mostly empty space

AMU

1/12 mass of Carbon 12

which two particles in an atom have relatively the same mass

Protons and Neutrons

A

mass number (P + N)

Z

atomic number (P)

X

atomic symbol

How do you find average atomic mass?

%₁(AMU₁) + %₂(AMU₂) = Average Mass (%₁+%₂=100)

Group 1A (Red)

soft, reactive (alkali) METALS

Group 2A (Orange)

alkaline earth metals

Group 7A (Purple)

halogens

Group 8A (Pink)

noble gasses

Where does the main group elements STOP on the right side of the periodic table?

Diagonally from Boron (B) to Astatine (At)

Empirical Formula

the smallest ratio of different elements in a formula (can represent many different compounds)

ways to draw molecules

structural, perspective, ball and stick, space filling

Ion

an atom that has become electrically charged

Poly-atomic Ion

a molecule that has become an Ion

which comes first in naming ionic compounds

cation

how do you dictate the charge of transitional metals?

Roman Numerals

NH₄⁺

Ammonium

H₃O⁺

Hydronium

Molecular Mass

sum of compounds atomic mass’

Molecular Formula

Gives you the actual number of atom in each element (i.e O₂, O₃, H₂O)

Molecular Compound

the sharing of electrons between two nonmetals

Ionic Compound

the transfer of electrons between a metal and nonmetal

Name diatomic molecules

H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂

Two or more nonmetals that form a compound

Molecular Compound

how do you name an non oxygenated anion in a ionic compound

by adding the suffix ‘ide’ to the root of the nonmetal

cation is to metal as anion is to

nonmetal

amu also equals

grams (g)/ mol (mole)

mole

number of atoms in exactly 12 grams of Carbon-12

form when certain gaseous compounds dissolve in water

Binary Acid Solutions

Binary Acid Solutions produce what

H⁺ when dissolved in water

for an oxoacid, the suffix ‘ate’ and ‘ite’ become

‘ic’ and ‘ous’

true of false: Formula mass is found differently than molecular mass

false

Avagadro’s # (N_a)

6.0221421 × 10²³ (items/mol)

mass %

(mass of element in a compound/mass of the full compound) x 100

what is the difference between a physical and chemical change

physical alters appearance but NOT chemical composition while chemical change creates new substances

how to extensive properties differ from intensive

the value of extensive properties are dependent on the amount while the value of intensive stay the same regardless of amount.

chemistry

study of materials and their transformations

matter

anything that occupies space

homogeneous mixture

uniform throughout (same proportions and composition) and only 1 phase

heterogeneous mixture

not uniform throughout (can see different substances and phases)

examples of physical properties

color, density, hardness, boiling point, etc

what are physical properties

properties observable without changing the substance

examples of chemical properties

reactivity and flammability

chemical properties

observable by transforming the substance into another substance (chemical change)

Law of multiple proportions

ratio of different atoms in a compound can be expressed as a ratio of small #’s