Name each of the following binary compounds, using the periodic table to determine whether the c

Name each of the following binary compounds, using the...

Key Concepts

Binary Compounds

Binary compounds are chemical compounds that contain exactly two different elements. They can be formed by either ionic or covalent bonding, depending on the elements involved. Understanding binary compounds is essential for naming and predicting the properties of the substance.

Ionic Compounds

Ionic compounds typically form between metals and nonmetals. Metals, which are found on the left side of the periodic table, tend to lose electrons and form positive ions, while nonmetals, found on the right side, gain electrons to form negative ions. The naming convention for ionic compounds involves stating the name of the metal first followed by the nonmetal with an 'ide' ending, and in cases where the metal can exhibit multiple oxidation states, a Roman numeral is used to indicate the specific charge.

Covalent (Molecular) Compounds

Covalent compounds are formed when two nonmetals share electrons instead of transferring them. Because both elements have similar tendencies to attract electrons, the compounds are typically molecular in nature. The naming of these compounds involves the use of prefixes to denote the number of atoms of each element present, which is a key difference from ionic compounds.

Oxidation States

Oxidation states refer to the charges that atoms are assumed to have when electrons are counted as belonging to the more electronegative element. In the context of nomenclature for ionic compounds, especially when transition metals are involved, knowing the oxidation state of the metal is crucial because it dictates the stoichiometry and way in which the compound is named, often using Roman numerals.

Nomenclature Rules

Nomenclature rules provide a systematic way to name chemical compounds so that their composition and structure can be inferred from their names. These rules differ for ionic and covalent compounds, with ionic compounds typically being named by stating the cation (usually a metal) followed by the anion (nonmetal with an 'ide' suffix), and covalent compounds being named with numerical prefixes to denote the number of atoms present.

Transcript

00:01 So we're going to be naming compounds that we don't know whether or not they're ionic or non -ionic to begin with.

00:07 To refresh how to tell a difference, let's go over a few things.

00:10 First of all, ionic compounds are formed between a metal and a non -metal.

00:19 On the other hand, non -ionic compounds are formed between two non -metals.

00:27 Then when we go on to naming them, both name the cation first and change the suffix.

00:37 Of the second element to ide.

00:42 On the ionic side we can use roman numerals if necessary to denote the charge of any transition metals and for non -ionic compounds we will use prefixes to denote how many of each element are present.

01:10 So to start with we can pull out our periodic table and we'll see that the line between metals and non -metals is here in red and all of the elements on this side are going to be non -metals and on this side they are metals.

01:31 We can tell the difference because of the different groups.

01:38 Now our first problem here is pbs2.

01:43 If we look we can find lead.

01:45 Pb right here a metal and s sulfur on the other side a non -metal therefore we can tell this is an ionic compound and we will start by naming the cadion lead and however lead is a transition metal that we need to denote the charge so we will calculate the charge sulfur is minus two because it is in group 16 two of those makes a minus 4 charge.

02:19 So the lead must have a plus 4 charge.

02:23 We'll write this as lead or sulfide.

02:30 Next, lead and sulfur again.

02:33 However, this time, there's only one sulfur, meaning minus 2 charge.

02:41 So the lead is plus 2 charge.

02:45 Similarly, we will write lead sulfide, but with 2 in roman numerals.

02:51 Instead.

02:54 Next we have silicon and oxygen...