test 2 Flashcards by Emily Askew

compounds

pure substances composed of atoms of two or more different elements chemically combined in fixed proportions

How well did you know this?

Not at all

Perfectly

ionic compounds

exist as aggregations of cations and anions held together by ionic bonds

How well did you know this?

Not at all

Perfectly

ionic bonds

attractive forces between positively and negatively charged entities

How well did you know this?

Not at all

Perfectly

formula units

the agreed upon unit of an ionic compound, consisting of the cations and anions in their smallest number ratio, linked together with ionic bonds

How well did you know this?

Not at all

Perfectly

monatomic ions

various ions formed from one atom

How well did you know this?

Not at all

Perfectly

Zinc charge

How well did you know this?

Not at all

Perfectly

Silver charge

How well did you know this?

Not at all

Perfectly

chromium charges, names, and older names

Cr2+, Chromium(II), Chromous

2. Cr3+, Chromium(III), Chromic

How well did you know this?

Not at all

Perfectly

iron charges, names, and older names

Fe2+, Iron(II), Ferrous

2. Fe3+, Iron(III), Ferric

How well did you know this?

Not at all

Perfectly

colbalt charges, names, and older names

Co2+, cobalt(II), Cobaltous

2. Co3+, cobalt(III), colbaltic

How well did you know this?

Not at all

Perfectly

copper charges, names, and older names

Cu+, Copper(I), Cuprous

2. Cu2+, Copper(II), Cupric

How well did you know this?

Not at all

Perfectly

Tin charges, names, and older names

Sn2+, Tin(II), Stannous

2. Sn4+, Tin(IV), Stannic

How well did you know this?

Not at all

Perfectly

Mercury charges, names, and older names

Hg2^2+, mercury(I), mercurous

2. Hg2+, mercury(II) mercuric

How well did you know this?

Not at all

Perfectly

lead charges, names, and older names

Pb2+, lead(II), plumbous

2. Pb4+, lead(IV), plumbic

How well did you know this?

Not at all

Perfectly

how are monotomic anions named

replacing the suffix on the parent atom name with “ide”

How well did you know this?

Not at all

Perfectly

polyatomic ions

“many atom” ions

How well did you know this?

Not at all

Perfectly

name and formula of acetate

C2H3O2^-

How well did you know this?

Not at all

Perfectly

name and formula of carbonate

CO3^2-

How well did you know this?

Not at all

Perfectly

name and formula of hydrogen carbonate (bicarbonate)

HCO2^-

How well did you know this?

Not at all

Perfectly

name and formula of hydroxide

OH^-

How well did you know this?

Not at all

Perfectly

name and formula of nitrite

NO2^-

How well did you know this?

Not at all

Perfectly

name and formula of nitrate

NO3^-

How well did you know this?

Not at all

Perfectly

name and formula of chromate

CrO4^2-

How well did you know this?

Not at all

Perfectly

name and formula of dichromate

Cr2O7^2-

How well did you know this?

Not at all

Perfectly

name and formula of Phosphate

PO4^3-

name and formula of hydrogen phosphate

HPO4^2-

name and formula of dihydrogen phosphate

H2PO4^-

name and formula of ammonium

NH4^+

name and formula of hypochlorite

ClO^-

name and formula of chlorite

ClO2^-

name and formula of chlorate

ClO3^-

perchlorate name and formula

ClO4^-

name and formula of permanganate

MnO4^-

name and formula of sulfite

SO3^2-

hydrogen sulfate (bisulfite)

HSO4^-

name and formula of sulfate

SO4^2-

name and formula of hydrogen sulfate

HSO4^-

name and formula of cyanide

CN^-

name and formula of peroxide

O2^2-

"ite" suggests

fewer oxygen atoms

"ate" suggests

more oxygen atoms

hydrates

ionic compounds which contain loosely associated water molecules

mono

tri

tetra

penta

hexa

hepta

octa

nona

deca

rules for naming molecular compounds

1. more metal like element is usually first. | 2. prefix of the first element followed by prefix name of second element with suffix changed to "ide"

acids

molecular compounds which release hydrogen cations when dissolved in water

binary acids

contain 2 different elements, hydrogen and one other nonmetal

hydrogen fluoride (HF) when a pure gas to dissolved in water

hydrofluoric acid

hydrogen chloride (HCl) when a pure gas to dissolved in water

hydrochloric acid

hydrogen bromide (HBr) when a pure gas to dissolved in water

hydrobromic acid

hydrogen iodide (HI) when a pure gas to dissolved in water

hydroiodic acid

molecular compounds

often composed of atoms of two or more nonmetals

oxyacids

compounds whose molecules contain hydrogen, oxygen, and one other elements

formula for nitrous acid

HNO2

formula for nitric acid

HNO3

formula for sulfurous acid

H2SO3

formula for sulfuric acid

H2SO4

formula for acetic acid

HC2H3O2

formula for hypochlorous acid

HClO

formula for chlorous acid

HClO2

formula for chloric acid

HClO3

formula for perchloric acid

HClO4

ite ending suggests

ous acid

ate ending suggests

ic acid

structural formulas

give most info as they depict the atom attachments

molecular formulas

give only the number of atoms of each type in one molecule of the compound, not the atom attachments

empirical formulas

give the least amount of info, the smallest whole number ratio of atoms of each type in one molecule

mole

Si unit of amount

Avogrados number

6.022 x 10^23

formula mass

the average mass of its molecules (if the compound was molecular) or the average mass of its formula units ( if the compound is ionic). it is simply the sum of all the atomic masses of all the same atoms in the molecule or formula unit

molar mass of a compound

the mass of one mole of its molecules (if the compound is molecular), or the mass of 1 mole of its formula units (if the compond is ionic)

mass percentage

percentage of the compounds total mass for which the element is responsible

limiting reactant

produces the least amount of product

excess reactant

left over product at end of a reaction

theoretical yield

maximum amt of product that can be made from specified amounts of reactants

actual yield

experimental amt of product made, always less than or = to the theoretical yield

percent yield

actual yield / theoretical yield x 100

solution

homogenous mixture

solute

the substance being dissolved

solvent

the substance doing the dissolving

aqueous solution

a liquid solution in which the solvent is water

concentration

an expression of how much solute is present

molarity formula

mol solute / liters of solution

most common way to express solution concentration

molarity

dilution equation

C1V1=C2V2

test 2 Flashcards

(93 cards)