chemistry

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average atomic mass formula

(mass)(%)+(mass)(%)/100

Calculating empirical formula

-Pretend that you have a 100g sample. That is, change % to grams. -Convert the grams to moles for each element. -Divide each number by the smallest number. -Multiply the result(if needed) to get rid of any fractions.

Acid Nomenclature

-ides go to hydro__ic acids -ates go to -ic acid -ites go to -ous acid -if hyper/per prefixes = keep same

Atomic Theory of Matter

1. all matter is made of atoms. 2. all atoms of an element are identical. 3. diff elements have diff atoms. 4. atoms keeps properties in chem reaction

1 mole of 12C has a mass of

12.000g

converting moles to a number

2 mol x 6.022 x 10^23 1 mol

PRACTICE: How many protons (p) and electrons (e) are found in a Se²⁻ ion?

34 p, 36 e Se has an atomic number of 34, so it contains 34 protons. The neutral atom would have 34 electrons, but because the ion has a -2 charge, this indicates that there are two additional electrons.

1 mole equals

6.022 x 10^23 of anything

chemical change

A change in matter that produces one or more new substances

polyatomic ion

A charged group of covalently bonded atoms

physical change

A physical change in a substance that does not change its identity

compound

A substance made up of atoms of two or more different elements

Metalloids are located

Along the zig zag line

Parallax

An apparent shift in the position of an object when viewed from different locations

matter

Anything that has mass and takes up space

Isotopes

Atoms of the same element that have different numbers of NEUTRONS (aka diff mass)

atom

Basic unit of matter

PRACTICE: Predict the chemical formula for the ionic compound formed by Ca²⁺ and ClO₃⁻

Ca(ClO₃)₂

Changes in states of matter

Condensation, Evaporation, Sublimation, Melting, Freezing

PRACTICE: Predict the chemical formula for the ionic compound formed by Cu²⁺ and P³⁻

Cu3Pu2

What are the diatomic elements?

H2, N2, F2, O2, I2 Cl2, Br2, Have No Fear Of Ice CoLd BeeR

atomic mass

Number of protons and neutrons

when multiplying/dividing sig figs

The answer must have the same amount of sig figs as the number with the least amount of sig figs in the question. Ex. 76.54x0.0086 = 0.66 <-- because 0.0086 only has 2 sig figs.

Oxyanion Nomenclature

When there are two oxyanions involving the same element: -The Fewest oxygens start with Hypo- and end in -ite -The 2nd fewest oxygens ends in -ite -The 2nd most oxygens ends in -ate. -The Most oxygens start with Per- and end in -ate

This is a:

chemical change

Molecular compounds are usually

composed of two or more nonmetallic elements

PRACTICE: What is the correct IUPAC name for CuNO₃?

copper (I) nitrate

when rounding off calculated answers, if the number is 5, round to the

even number

periodic table columns are

groups

protons and neutrons are the only particles that

have a charge

PRACTICE: What is the correct IUPAC name for HCN(aq)?

hydrocyanic acid

When atoms lose or gain electrons they become

ions

formula weight (FW)

is the sum of the atomic weight (AW) of atoms in the chemical formula of a substance

protons and neutrons have essentially the same

mass

Density is

mass/volume

ionic compounds are formed between

metals and nonmetals

Anions

negatively charged ions (gain electrons) (right side)

PRACTICE: What is the correct IUPAC name for HNO₃(aq)?

nitric acid

periodic table rows are

periods

H20 (l) --> H20 (s) is a

physical change

Cation

positively charged ion (lost electrons) (left side)

Nonmetals are located

right

PRACTICE: What is the correct IUPAC name for Ag₂S?

silver sulfide

elements in the same group have

similar chemical properties

homogeneous mixture is also called a

solution

Density is the physical property of a

substance

PRACTICE: What is the correct IUPAC name for As₄O₃?

tetrarsenic trioxide

molar mass

the mass of one mole of a substance

Atomic number

the number of protons in the nucleus of an atom

percent composition

the percent by mass of each element in a compound

emperical formula

the smallest whole number ratio of the atoms in a compound

molecular weight (MW)

the sum of the atomic weights of its atoms

When adding/subtracting sig figs

use the same number of decimal places as the measurement with the fewest decimal places


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