Nomenclature

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Nomenclature

Drawing

Bohr Rutherfords

These are diagrams that show elements electrons from the inner to the outer shell An electron has two electrons in it's first, eight in the second eight in the third and then it gets more complicated from their. You draw lines from the outer shell to the shell of the other atom when drawing it for bonds and compounds.

Lewis Dot diagrams

These are simpler diagrams than bohr rutherfords. You only draw the valence electrons, in dots around the chemical symbol. And then draw connections with arrows to show if an electron has been lost or gained when being used for compounds.

Example

Lewis Structures

Lewis structures are a simple ways for showing the valence shells in an atom. These are usually used when drawing molecular compounds. Draw lines to the atoms to show they are being shared.

Example: Carbon Dioxide

Indicating Charge

Factoring

Factor out the numbers to reduce them to the lowest possible value. If they don't have one you can just leave it alone.

Example: Octane

Criss Cross

Cross the charge from the second element to the other and vice versa, this will help you determine the number of atoms in a compound. This is the method I prefer as I believe it's the fastest.

Example: Sodium Phosphide

If it's a multivalent un cross the numbers to get their charge they specify the multivalent metal by indicating it's charged by a roman numeral.

Zero Sum

Find the number of atoms that would balance it out. that cancel out to zero between the numbers, and that will be your final answer. Say you have something with a positive +4 charge and a -5 charge. You would need 5 of the first and 4 of the second to make the sum of them both multiplied together to be zero.

Periodic Table

Something to show you all the elements on the periodic table. The colors indicate what kind of element it is, check the legend below it. (To expand, hover your cursor over the image then click the expand icon that appears in the top right corner).

Formulas

When writing formulas for compounds the metal goes before the non metal if there's one. And place the number of atoms used in the compound after the chemical symbol.

Ex. Octane= C8H18

Elements

Noble Gases

The noble gases are in a gaseous form at room temperature. There are seven of them, an example being neon. They have a complete outer shell, so they usually don't combine with other elements.

Non-metals

Are elements that gains electrons rather than losing them. Since they absorb electrons they become negatively charged as they have more electrons than protons. They are the anion of a bond, so they are named after the metal.They are on the right side of the periodic table.

Multivalent Metal

A Multivalent Metal is a metal that could have different valence electrons. Indicate the number of valence electrons it has with a roman numeral. One for each valence electron.

Metals

Metals are elements that lose their electrons. And because they lose electrons they are positively charged as they now have more protons than electrons. They are the cation of a bond, so they are named before the metal. They are on the left side of the periodic table. With the exception of hydrogen which is a non-metal.

Diatomics

Diatomic elements are elements that can't exist on their own. Meaning that they must have two elements to exist. But it could be another one of itself though. Like Nitrogen, nitrogen is N2 because N1 cannot exist. But they can also bond with other elements to complete themselves, like Carbon Monoxide, as oxygen is a diatomic as well and uses the carbon to complete itself. And yes, this is a molecular bond, as they are both non-metals.

Compounds

Molecular

Molecular compounds are compounds that are not made up of a metal and non- metal. And they share electrons rather than losing or gaining them. They share their electrons since they are nonmetals.

Example: Water

They share electrons they don't lose or gain them.

Ionic

Ionic basic

Basic Ionic compounds are the metals and non metals, which is the most simple kind of compound, and remember that you write the metal before the non-metal.

Ex. Sodium Chloride=NaCL

Multivalent

They are compounds that have metals that have more than one possible valence charge to them. Determine the charge before writing the formula by uncrossing the number of each element in the formula and indicate the multivalent metal by placing a roman numeral in front of it.

Ex. FeO=Iron(II) Oxide

Polyatomics

Polyatomic compounds are compounded with more than two atoms.Usually this is with oxygen. Such as chlorate, which is CLO3. When naming polyatomics, you add the suffix ate instead of -ide to indicate that it is polyatomic.

Ex.Phosphate= PO4

Covalent

Is a compound created by a covalent bond when they share electrons. These are when you add the special endings on two the names of the compounds. Depending on the number of atoms it determines your prefix, that goes on both the metal and non-metal. You don't add a prefix if the first element has one though.

Prefixes

Ex. Carbon Dioxide CO2 Dihydrogen Oxide. H2O Fancy name for water.