What are the rules on naming covalent compound?

Answer 1

Rules of writing formulas: * · positive ion is written first … this is usually a metal * · negative ion is written second … this is usually a nonmetal * · subscripts are used to show how many ions of each part are in the compound. They are used to balance the charge of the ions.

Answer 2

Rule 1: CRISS-CROSS rule

1. write the correct symbols of the elements and radicals
2. Above each symbol, write the correct valence or oxidation numbers.
Ex. Al+3 O-2
3. To obtain the proper subscript, criss-cross the valence or oxidation
number,and drop the algebraic sign.
Ex. Al+3O-2 became Al2O3

Rule 2: When the subscript is number 1, subscript is not written.
Ex. Sodium Chloride- Na+1 Cl+1 --- NaCl

Rule 3: When the oxidation # of both elements are numerically equal but grater than 1, the subscript are not also written.
Ex. Calcium Oxide~ Ca+2O-2 ----- CaO

Rule 4: All radicals tke more than once( the subscript is 2 or more) must be
enclosed in Pahrentheses().

Ex. Ammonium Sulfate NH4+1 SO4-2-----(NH4)2 SO4

RULE 4: All subscripts must be reduced to lowest term (except for molecular or
covalent copound).

Ex. Tin (IV) Chloride ~ Sn+4Cl-1------ SnO2

*ANOTHER RULE*

Write the symbol for the atom or polyatomic ion with the positive oxidation number first.

Ex. Al+3

Follow this with the symbol of the atom or polyatomic ion with a negative oxidation number.

Ex. I-1

Use subscripts to make the sum of the oxidation numbers equal to the charge of ions.

Ex. Al+3 and I-1

We write AlI3

When a subscript is used with an ion containing two or more elements, the ion must be enclosed in parentheses () before writing the subscript.

Ex. Mg+2 and NO3-1

is written as Mg (NO)

Answer 3

you have to know how much each element weighs, aka its molar mass. based on how much information they give you, you write the element symbol and then the number of times that element shows up in a small subscript number to the right of it. you also have to put the element symbols in alphabetical order. for example if you are told that you have some mix of oxygen and hydrogen and its molar mass is 18, you know you have water or H2O, because oxygen weighs 16 and hydrogen weighs 1 and that's the only formula you could have with those two elements and that weight. You don't write OH2 because that's not in alphabetical order. You know it's not HO because that would only weigh 17 grams per mole.

Answer 4

To write the formula for an ionic compound , firstly write the symbols of the elements. Then determine the charge on each element and finally from the known charges determine the subscripts that will equalize the total positive and negative charge so that the compound becomes electrically neutral .

Answer 5

Naming covalent bonds mainly involves the use of Greek numeral prefixes (NP), according to how many atoms there are of each element. As a general rule of thumb, the name of the leastelectronegative element is first, then the name of the mostelectronegative element. This is similar to how other compounds are set up or written, as in cation (positive ion) first and anion (negative ion) second

(Cation + Anion).

1 = mono*

2 = di

3 = tri

4 = tetra

5 = penta

6 = hexa

7 = hepta

8 = octa

9 = nona

10 = deca

*is never used for the first element, is seldom used for the second element.

Also, the suffix or ending "-ide" is added to the most electronegative element or the second element named. The ending of the first element named doesn't change, only the prefix or beginning. Both the prefix and the suffix are changed for the second element.

Ex. CO2 is Carbon Monoxide (one case where mono is used for the second element) instead of Carbon Monoxygen.

NPelement1 + NPelement2-ide

(Cation + Anion-like setup).

Another way to look at the least vs most electronegative order as a general rule is to see which element is further left on the Periodic Table (less electronegative) or further right on the periodic table (more electronegative).

least electronegative = further left

most electronegative = further right

Steps

1. Place names of elements in order accordingly, and also placing appropriate prefixes according to number of atoms of each element.

least electronegative + most electronegative

2. Add suffix "-ide" to ending of second element accordingly.

Answer 6

First, you need to name the first element. You can look it up on the Periodic Table of Elements. Then name the second element by using its root + suffix. (Note: -ide is most often used.)

For example: NaCl

Na is Sodium

Cl Chlorine

But since it is Cl second element it should be chloride.

Answer: Sodium chloride

(Note: sometimes you need to add prefixes)

CO2-- Carbon dioxide. If you are wondering why it shouldn't be just oxide, it is because the subscript is two, which means the oxygen has 2 atoms. That's why we used prefix di-.A Greek prefix which means two. (You can look up the different greek prefixes on the internet if you want.

-For acids that contain Hydrogen hydro + the suffix -ic is attached to the root then add acid in the end.

Example: HCI- Hydrochloric acid

H2SO4- Sulfuric acid

NOTE: The First letter in the first element should be capitalized. While the first letter in the second element should be small.

Answer 7

The biggest and perhaps only rule is to balance the equation. Make sure that the number of atoms of each element are the same on each side (unless there's some sort of nuclear reaction occuring). Number of atoms in an element are written subscript on the right of the element. The number of molecules is written to the left of the molecule.

eg.

1C6H12O6 + 6O2 <--> 6CO2 + 6H20 + energy

Note:

6 C on each side

12 H on each side

18 O on each side

while energy appears to be a new term that unbalances the equation, it is merely hidden on the left hand side. The energy is located in the bonds between the atoms within the molecule.

Answer 8

The left side of the chemical formula is the reactant and the right side is the product. For example

Hydrogen + Oxygen -----------> Water

Answer 9

what are the rules in writing chemical symbols?

for you all out there that know this answer can you please help me this is for a chemisty work shop