Chemistry chapter 7

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Mercury (I) ion (Mercurous ion)

*Hg2 2+

Hydrogen combined with a nonmetal

+1

Hydrogen combined with a metal

-1

only charge on Ag

1+

typical charge on group 1 metals

1+

Binary Ionic Compound Formulas

1. Metal written first Nonmetal written second 2. Use criss-cross method and subscripts to insure sum of charges = 0

only charge on Zn

2+

typical charge on group 2A metals

2+

only charge on Al

3+

empirical formula

A formula showing the lowest whole number ratio of atoms in a compound; (symbols for elements combined in a compound; subscripts show smallest whole-number mole ratio of different atoms in a compound)

Binary acids

Acids that consist of two elements, usually hydrogen and 1 halogen

Oxyacids

Acids that contain hydrogen, oxygen, and a third element (usually a nonmetal )

Molecular formula

Actual formula of a molecular compound

AlH₃

Aluminium Hydride

AlP

Aluminium Phosphide

Al(HSO₃)₃

Aluminum Bisulfite

Al₂(CO₃)₃

Aluminum Carbonate

Al3+

Aluminum ion

NH₄NO₃

Ammonium Nitrate

(NH₄)₂O₂

Ammonium Peroxide

(NH₄)PO₄

Ammonium Phosphate

(NH₄)₂S

Ammonium Sulfide

salt

An ionic compound composed of a cation and the anion from an acid

Binary Acids

Are acids that consist of two elements, usually hydrogen, and one of the halogens.

Oxyacids

Are acids that contain hydrogen, oxygen, and a third element usually a nonmetal.

AsCl₃

Arsenic Trichloride

Ions with greater number of oxygen atoms ends in

Ate

Covalent-network compounds

Atoms covalently bonded in a 3-D network

write the empirical formula for Ba²⁺ + Cl⁻

BaCl₂

Ba(ClO)₂

Barium Hypochlorite

Ba2+

Barium ion

BeI₂

Beryllium Iodide

Be2+

Beryllium ion

Bi(HSO₄)₃

Bismuth(III) Bisulfate

Br-

Bromide

Cd(NO₃)₂

Cadmium Nitrate

Ca(HSO₄)₂

Calcium Bisulfate

Ca2+

Calcium ion

CsBrO₃

Cesium Bromate

CsCN

Cesium Cyanide

CsNO₂

Cesium Nitrite

Cs+

Cesium ion

Cl-

Chloride

Cr(NO₃)₃

Chromium(III) Nitrate

Cr₂(SO₄)₃

Chromium(III) Sulfate

Cobalt (II) ion (Cobaltous ion)

Co2+

Cobalt (III) ion (Cobaltic ion)

Co3+

Co(ClO₃)₂

Cobalt(I) Chlorate

CoCl₂

Cobalt(II) Chloride

Co(HSO₃)₄

Cobalt(IV) Bisulfite

CoF₄

Cobalt(IV) Fluoride

Co3+

Cobaltic Cobalt(I II)

Binary ionic compound

Compounds of 2 elements

CuBr

Copper(I) Bromide

Cu₂CO₃

Copper(I) Carbonate

CuCl₂

Copper(II) Chloride

CuSO₄

Copper(II) Sulfate

Chromium (II) ion (Chromous ion)

Cr2+

Chromium (III) ion (Chromic ion)

Cr3+

Copper (I) ion (Cuprous ion)

Cu+

Copper (II) ion (Cupric ion)

Cu2+

Cu2+

Cupric

Cu(ClO₄)₂

Cupric Perchlorate

Cu+

Cuprous copper1

Iron (II) ion (Ferrous ion)

Fe2+

Iron (III) ion (Ferric ion)

Fe3+

Fe3-

Ferric

Fe2-

Ferrous

F-

Floride

C and Si

Form covalent bonds

Do Transition Metals for Cations or Anions?

Form positive ions (cations), but not always with the same charge.

Au(ClO₄)₃

Gold(III) Perchlorate

mono

Greek prefix for 1 with covalent bonding

deca

Greek prefix for 10 with covalent bonding

di

Greek prefix for 2 with covalent bonding

tri

Greek prefix for 3 with covalent bonding

tetra

Greek prefix for 4 with covalent bonding

penta

Greek prefix for 5 with covalent bonding

hexa

Greek prefix for 6 with covalent bonding

hepta

Greek prefix for 7 with covalent bonding

octa

Greek prefix for 8 with covalent bonding

nona

Greek prefix for 9 with covalent bonding

Mercury (II) ion (Mercuric ion)

Hg2+

H-

Hydride

H₂O₂

Hydrogen Peroxide

H₂SO₄(aq)

Hydrogen Sulfate

H+

Hydrogen ion

H₃PO₄(aq)

Hydrogen phosphate

Ion with 1 fewer oxygen atom than ite has the prefix

Hypo

-ite (tiny like a mite)

In oxyanions: The ion with less oxygen is given the ending: -

-ate (I ate too much; more)

In oxyanions: The ion with more oxygen is given this ending: -

hypo-

In oxyanions: The ion with one less less oxygen is given the beginning: ____-

per-

In oxyanions: The ion with one more more oxygen is given the beginning:

I-

Iodide

Oxidation Number =

Ion Charge - number of electrons transferred to or away from an atom when it becomes an ion.

Salt

Ionic compound composed of a cation and the anion from an acid

Fe₂O₃

Iron (III) Oxide

FeBr₂

Iron(II) Bromide

FeCO₃

Iron(II) Carobonate

FeCrO₄

Iron(II) Cromate

Fe(PO₄)₂

Iron(II) Phosphate

Fe₂(Cr₂O₇)₂

Iron(III) Dichromate

Ion with smaller number of oxygen atoms end in

Ite

Pb(HCO₃)₂

Lead(II) Bicarbonate

Pb(ClO₄)₂

Lead(II) Perchlorate

PbO₂

Lead(II) Peroxide

LiClO₃

Lithium Chlorate

LiH

Lithium Hydride

LiOH

Lithium Hydroxide

Li₃PO₄

Lithium Phosphate

Li+

Lithium ion

Mg(HSO₃)₂

Magnesium Bisulfite

Mg(ClO₂)₂

Magnesium Chlorite

MgCr₂O₇

Magnesium Dichromate

Mg₃N₂

Magnesium Nitride

Mg2+

Magnesium ion

Hg2+

Mercuric

Hg1+

Mercurous

Hg₂(C₂H₃O₂)₂

Mercury(I) Acetate

Hg₂CrO₄

Mercury(I) Chromate

Hg₂SO₄

Mercury(I) Sulfate

HgCL₂

Mercury(II) Chloride

Criss-Cross Method

Method used to insure that there is a balance between the number of electrons transferred by the metal to the nonmetal.

Manganese (II) ion (Manganous ion)

Mn2+

Manganese (III) ion (Manganic ion)

Mn3+

write the formula for Na⁺ + Cl⁻

NaCl

Anions

Negative ions

Ni(ClO₃)₂

Nickel(II) Chlorate

NiSO₃

Nickel(II) Sulfite

Nonmetal Anion Names end in __________

Nitride (N³⁻), Phosphide (P³⁻), Oxide (O²⁻), Sulfide (S²⁻),Fluoride (F¹⁻), Chloride (Cl¹⁻), , Bromide (Br¹⁻), , Iodide (I¹⁻)

Negative Ion (anion) Formation

Nonmetals tend to gain valence electrons to become stable and form negative ions called anions.

Oxidation numbers

Number of electrons that must be added to or removed from an atom in a combined state to convert the atom into the elemental form

In order to become stable, atoms will either gain or lose valence electrons in order to acquire an _________. (like a Noble Gas)

Octet.

O2-

Oxide

Lead (II) ion (Plumbous ion)

Pb2+

Lead (IV) ion (Plumbic ion)

Pb4+

Ion with 1 or more oxygen atoms than -ate has the prefix

Per

Percentage composition

Percentage by mass of each element in a compound

Pt(CN)₄

Platinum(IV) Cyanide

Pb4+

Plumbic Lead(IV)

Pb2+

Plumbous Lead (II)

Oxyanions

Polyatomic anions that contain oxygen

Common Polyatomic Ions

Polyatomic ions have their own names and charges and must either be memorized or looked up on a chart

Cations

Positive ions

KClO₃

Potassium Chlorate

KMnO₄

Potassium Permanganate

K+

Potassium ion

Rb₂CrO₄

Rubidium Chromate

Chemical formulas

Show relative number of atoms in a chemical compound

AgI

Silver Iodide

Ag₂SO₃

Silver Sulfite

Ag+

Silver ion

Tin (II) ion (Stannous ion)

Sn2+

Tin (IV) ion (Stannic ion)

Sn4+

NaHSO₄

Sodium Bisulfate

Na₂Cr₂O₇

Sodium Dichromate

Na₂SO₄

Sodium Sulfate

Sn4+

Stannic Tin(IV)

Sn2+

Stanous Tin(II)

Sr₃(PO₄)₂

Strontium Phosphate

SrS

Strontium Sulfide

S2-

Sulfide

Formula mass

Sum of the average atomic mass of all atoms represented in a formula

Molar mass

Sum of the masses of the element in one mole molecules or formula units that make up a compound

Empirical formula

The symbol of element in a compound with subscripts showing the smallest whole number mole ratio of the atom in the compound

SnF₄

Tin (IV) Fluoride

Sn₃(PO₄)₂

Tin Phosphate

SnBr₂

Tin(II) Brimide

SnO

Tin(II) Oxide

Sn(MnO₄)₄

Tin(IV) Permanganate

Sn(SO₄)₂

Tin(IV) Sulfate

Ionic Compound Formation

Total number of electrons transferred by the metal must equal the total number of electrons accepted by the nonmetal.

The reactivity of an atom is related to its _________ electrons

Valence

ZnCr₂O₇

Zinc Chromate

Zn(CN)₂

Zinc Cyanide

ZnNO₂

Zinc Nitrite

crystal lattice

a 3-dimensional geometrical structure formed by the alternative arrangement of positive and negative ions Shown above: crystal lattice of NaCl.

Oxyanion

a polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms

CH3COO-

acetate

NH4+

ammonium

what is an ion

an atom that has either gained/lost electrons

Monatomic ion

an ion formed by only one atom

monatomic ion

an ion formed from a single atom. (remember to change nonmetals to -ide ending)

Polyatomic ions

an ion made up of two or more atoms bonded together that acts as a single unit with a net charge

Anion

an ion with a negative charge

Cation

an ion with a positive charge

Electrolyte

an ionic compound whose aqueous solution conducts an electric current

name of ions with - charges

anions "a nEGATIVE ion"

ions

atoms that have acquired either a positive or a negative charge.

Formation of an Ionic Bond

between a metal that loses one or more valence electrons and a nonmetal that gains one or more valence electrons.

CO3-

carbonate

name of ions with + charges

cations "c a + ion"

Formula Unit

chemical formula for an ionic compound; simplest ratio of positive to negative ions; overall charge = 0

binary compounds

compounds composed of two different elements; (compounds of 2 elements between metal (positive, s-block and p-block) and nonmetal (negative); metal is always listed first; change nonmetal to -ide ending)

Acid

distinct type of molecular compound; would show up on pH scale as a value below 7

HcO3-

hydrogen carbonate ( bicarbonate )

OH-

hydroxide

Monatomic ions

ions formed from 1 atom

Polyatomic Ions

ions made up of more than one atom; acts as an individual ion in a compound; charge applies to entire group of atoms.

Stock system

it is a widely used system of chemical nomenclature developed by the german chemist Alfred Stock. In this system, the oxidation states of some or all the elements in a compound are indicated in parentheses by Roman numerals

Differentiate between molecular and ionic compounds

metal + non-metal = ionic compound non-metal + non-metal = molecular compound

Positive Ion (Cation) Formation

metals tend to lose valence electrons to become stable and form positive ions called cations

nomenclature

naming system

NO3-

nitrate

binary molecular compounds

nonmetal to nonmetal; covalent bonds; uses Greek prefixes

Monatomic Ions

one-atom ions

( PO4 )3-

phosphate

oxyanions

polyatomic ions that contain oxygen

Stock system

specifically used for d-block elements, use Roman numeral to describe charge of metal, use periodic charge to find charge of nonmetal

Properties of Ionic Compounds

strong attraction between oppositely charged ions means: high melting & boiling points ionic crystals are very hard but brittle conduct electricity when dissolved in solution or melted (ELECTROLYTES)

If the metal loses more electrons than the nonmetal gains,then __________ must be used to balance the charges

subscripts.

( SO4 )2-

sulfate

oxidation states

the condition of an atom expressed by the number of electrons that the atom needs to reach its elemental form

Ionic bond

the electrostatic force that holds oppositely charged particles together in an ionic compound

Lattice energy

the energy required to separate one mole of the ions of an ionic compound, which is directly related to the size of the ions bonded and is also affected by the charge of the ions

Chemical bond

the force that holds two atoms together; may form by the attraction of a positive ion for a negative ion or by sharing electrons

Alloy

the mixture of elements that has metallic properties; most commonly forms when the elements are either similar in size, or the atoms of one element are much smaller than the atoms of the other

Oxidation numbers

the number assigned to an element that shows how many electrons it gains, loses, or shares

percentage composition

the percentage by mass of each element in a compound

Oxidation number

the positive or negative charge of a monatomic ion

Formula unit

the simplest ratio of ions represented in an ionic compound

formula mass

the sum of the average atomic masses of all atoms represented in the formula of any molecule, formula unit, or ion

Greek prefixes

used to name molecules with covalent bonds


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