Compounds

Metallic Bond

This is a type of chemical bond that forms among metallic substances and is a direct consequence of attractive electrostatic forces between the negatively charged sea of delocalized electrons and the positively charged metal ions.

• In solid metals, individual metal atoms are so close to one another that the electron cloud of one metal atom overlaps with its neighboring metal atom.

• This creates the “sea of delocalized electrons.” In other words, the electrons are free to wander within the crystal structure.

Covalent bond

is a type of chemical bond wherein the electrons involved in bond formation are shared by the two atoms bonded with one another.

• This type of bond is designated by a “dash” connecting one atom to another.

• Each of this is composed of two electrons, and each atom being bonded covalently contributes one electron to that bond.

ionic bond

It is a type of chemical bond which involves the complete transfer of valence electron(s) between atoms. This bond usually occurs between a metal and a nonmetal.

• The transfer of electrons is made possible because metals tend to lose their valence electron(s) to become a positively-charged cation.

• In contrast, the nonmetals tend to gain the electron(s) lost by the cations to become a negatively-charged anion.

• The bond results from the attraction of the two oppositely charged substances.

Coordinate Covalent Bond

It is also known as a dative bond. In this type of chemical bond, both electrons are supplied by one of the two bonded atoms. This is commonly observed among __________ compounds and inorganic complexes and is written just like a covalent bond.

binary covalent compound

It is a covalent compound that is made up of exactly two elements only.

The first element

In the rules of naming binary covalent compounds which of the two elements in the chemical formula is named first using the name of that element.

The second element

In the rules of naming binary covalent compounds, which of the two elements in the chemical formula is named as if it is an anion.

Prefix

In the rules of naming binary covalent compounds, the number of that element must be indicated using the appropriate _____.

Mono-

In the rules of naming binary covalent compounds, this prefix must never be used in denoting the number of the first element.

drop

In the rules of naming binary covalent compounds, If the name of the element starts with a vowel, _____ the “a” or “o” in the prefix. 

1

The prefix Mono- stands for which number

2

The prefix Di- stands for which number

3

The prefix Tri- stands for which number

4

The prefix Tetra- stands for which number

5

The prefix Penta- stands for which number

6

The prefix Hexa- stands for which number

7

The prefix Hepta- stands for which number

8

The prefix Octa- stands for which number

9

The prefix Nona- stands for which number

10

The prefix Deca- stands for which number

Identiify the chemical symbol of the element

In the rules of writing the chemical formula of binary covalent compounds, firstly, we must ______?

subscript

In the rules of writing the chemical formula of binary covalent compounds, take note of the prefix used for each element, and write the corresponding number as a _______ of that element.

less electronegative

In the rules of writing the chemical formula of binary covalent compounds, we must write the _______ element first. The most electronegative element in the periodic table is fluorine (F). Hence, you can make it a convention that the farther the element is from fluorine, the less electronegative it is.

binary ionic compound

It is a compound that is composed of a single type of cation and a single type of anion.

Type I binary ionic compound

It is a type of binary ionic compound in which the cation exhibits only one oxidation state.

Type II binary ionic compound

It is a type of binary ionic compound in which the cation exhibits at least two oxidation states

cation, anion

In the rules of naming binary ionic compounds, the ______ is always named first, while the _____ is always named second.

cation, anion

In the rules of naming binary ionic compounds, Monoatomic ___ are named as if they are elements. Meanwhile, the monoatomic ___ takes the root of the element name + –ide. 

have special and unique names

In the rules of naming binary ionic compounds, polyatomic cations and anions ________, and you should familiarize yourself with them.

not usually used in the nomenclature of ionic compounds.

In the rules of naming binary ionic compounds, The prefixes used in the nomenclature of covalent compounds are ________…?

ammonium

NH₄⁺

hydroxide

^–OH

acetate

C₂H₃O₂^–

nitrate

NO₃^–

nitrite

NO₂^–

cyanide

CN^–

permanganate

MnO₄^–

peroxide

O₂^2–

thiosulfate

S₂O₃^2–

hypochlorite

ClO^–

chlorite

ClO₂^–

chlorate

ClO₃^–

perchlorate

ClO₄^–

sulfate

SO₄^2–

hydrogen sulfate/bisulfate

HSO₄^–

sulfite

SO₃^2–

hydrogen sulfite/bisulfite

HSO₃^–

carbonate

CO₃^2–

hydrogen carbonate/bicarbonate

HCO₃^–

chromate

CrO₄^2–

dichromate

Cr₂O₇^2–

arsenate

AsO₄^3–

phosphite

PO₃^3–

phosphate

PO₄^3–

hydrogen phosphate/biphosphate

HPO₄^2–

dihydrogen phosphate

H₂PO₄^–

cation, anion

In the rules of naming Type II binary ionic compounds, The ____ is always named first, while the ____ is always named second.

The systematic method

In the rules of naming Type II binary ionic compounds, This method states that in naming the cation, identify the oxidation state of the cation, and write the oxidation state (in roman numeral) adjacent to the name of the cation.

Anion

In the rules of naming Type II binary ionic compounds, we name the monoatomic _____ by taking the root of the element name + –ide. Use corresponding names for polyatomic anions.

not usually used in the nomenclature of ionic compounds.

In the rules of naming Type II binary ionic compounds, the prefixes used in the nomenclature of covalent compounds are _______?

stock system

In the rules of naming Type II binary ionic compounds, In naming the cation using the ________, identify the oxidation state of the cation. If the oxidation state of the cation is less than the other oxidation state, the cation is named as the element root name + –ous. On the other hand, if the oxidation state of the cation is greater than the other oxidation state, the cation is named as the element root name + –ic.

Pb²⁺

• Stock Name: plumbous

• Systematic Name: lead(II)

Pb⁴⁺

• Stock Name: plumbic

• Systematic Name: lead(IV)

Fe²⁺

• Stock Name: ferrous

• Systematic Name: iron(II)

Fe³⁺

• Stock Name: ferric

• Systematic Name: iron(III)

Co²⁺

• Stock Name: cobaltous

• Systematic Name: cobalt(II)

Co³⁺

• Stock Name: cobaltic

• Systematic Name: cobalt(III)

Cu⁺

• Stock Name: cuprous

• Systematic Name: copper(I)

Cu²⁺

• Stock Name: cupric

• Systematic Name: copper(II)

Acids

These are compounds that release (directly or indirectly) free H₃O⁺ in an aqueous solution.

Ternary Acid (Oxoacid/Oxyacid)

These refer to inorganic acids that contains oxygen.

Binary Acid

These refer to inorganic acids that does not contain oxygen.

Hydrohalic Acids

These are acids in which hydrogen is combined with a halogen.

Hydrohalic Acids

This type of acid has a nomenclature where The prefix hydro is added to the modified anion name ending in -ic as acid is also added to it.

Ternary Acid that has a Low Oxidation State

This is a type of Ternary Acid where the anion ends with -ite. Therefore its nomenclature is a modified anion name ending with -ous with acid added to it.

Ternary Acid that has a High Oxidation State

This is a type of Ternary Acid where the Anion ends with -ate. Therefore its nomenclature is a modified anion name ending with -ic with acid added to it.

hypochlorite

ClO^–

chlorite

ClO₂^–

chlorate

ClO₃^–

perchlorate

ClO₄^–

hypobromite

BrO^–

bromite

BrO₂^–

bromate

BrO₃^–

perbromate

BrO₄^–

hypoiodite

IO^–

iodite

IO₂^–

iodate

IO₃^–

periodate

IO₄^–

indicating their correct charge.

In the rules writing the chemical formula of type 1 Binary Ionic Compounds, separately write the cation and anion, whilst also ______?

In the rules writing the chemical formula of type 1 Binary Ionic Compounds, this method states that you must take the absolute value of the charge of the cation, and write it as a subscript of the anion. In the same way, take the absolute value of the charge of the anion and write it as the subscript of the cation.

parenthesis

In the rules writing the chemical formula of type 1 Binary Ionic Compounds, For polyatomic ions, write __________ if necessary.

The subscripts of the anion and cation must be written in the lowest possible terms.

In the rules writing the chemical formula of type 1 Binary Ionic Compounds, As an example, the formula of ferrous sulfate is written as FeSO₄, instead of Fe₂(SO₄)₂ since the subscripts of both ions are 2. In the same manner, the formula of tin(IV) sulfate is Sn(SO₄)₂ instead of Sn₂(SO₄)₄.

State which rule is this in writing the chemical formula of Binary Ionic Compounds.

oxidation number

It is a number (positive, negative, or zero) assigned to a certain element to indicate its degree of oxidation or reduction.

0

In the rules of assigning Oxidation numbers, Free/uncombined elements have oxidation numbers equal to __. Example: H₂, Al, Fe, Zn, and N₂ all have _ oxidation numbers.

equal

In the rules of assigning Oxidation numbers, Monoatomic ions have oxidation numbers that are always ____ to their charge. Example: The oxidation number of Fe²⁺ is +2, and the oxidation number of Cl^– is -1.

+2

In the rules of assigning Oxidation numbers, In its ionic form, the oxidation number of Group I elements (except H) is always +1, while the oxidation number of Group II elements is always __.

-1

In the rules of assigning Oxidation numbers, The oxidation number of H is +1. However, when combined with metal in hydride compounds, its oxidation number is __. Example: In lithium hydride, LiH, the oxidation number of H is __.

+3, -1

In the rules of assigning Oxidation numbers, in all of its compounds, Al has an oxidation number of _. Also, F has an oxidation number of _ in all of its compounds.

-1

In the rules of assigning Oxidation numbers, The oxidation number of oxygen is -2, except for hydrogen peroxide (H₂O₂) or peroxide anion (O₂^2–), wherein its oxidation number is __.

Halogens

In the rules of assigning Oxidation numbers, this group within the periodic table have negative oxidation numbers when it forms halide compounds. However, when it forms oxygen-containing compounds, its oxidation number is positive.