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An ionic compound is a chemical compound made of ions held together by electrostatic forces. The overall charge of the compound is neutral, but consists of cations (positive charge) and anions (negative charge). In the ionic compound name, the metal is named first and the nonmetal is second and the ending changes ide. To find the ionic formula- ___(# of metals)(charge +) + ___(# of nonmetals)(charge -)=0

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An ion is an atom or a molecule which the number of electrons is not equal to the number of protons, giving the atom or molecule a positive or negative charge. It forms when atoms gain or loose an electron. Also, cations have a positive charge, and anions carry a negative charge.

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Diatomic Molecules are composed of two of the same atoms bonded together. On the Periodic Table, the diatomic molecules can be found in "Super Seven."

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Metals:
-Metals are located in the left hand center
-Good conductors of heat and electricity, malleable, ductile, lustrous, and mostly solid at room temperature

Nonmetals:
-Nonmetals are located in the upper right hand corner
- Poor conductors of heat and electricity
-They lack most properties of metals

Metalloids:
-Metalloids are six elements on a diagonal line
-Called semimetals or semiconductors because their conductivity is between that of metals and nonmetals.
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Alkali Metals- group 1
Alkaline Earth Metals- group 2
Transition Metals- group 3-11
Halogens- group 17
Noble Gases- group 18
Lanthanides
Actinides

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The periodic table lists all of the known elements in order of their atomic # and in columns that depend on similarities in their chemical and physical properties.

Vertical Column= group (families)
Horizontal Row= period

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When writing an Isotope, there must be a subscript on the bottom left side, which tells you the atomic number and the number of protons and electrons. There also must be a number on the top left, which is referred as the superscript. The superscript provides the mass number, which is the number of protons and neutrons combined.

When you write the name of the Isotope you write the name of the element followed by a dash, and then put the mass number.

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Isotopes are atoms of an element with the same number of protons and different number of neutrons and mass number.

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What is a Chemical Formula?

We encounter chemical substances and compounds everyday. The substances under the kitchen sink that we use to clean our houses as well as those that are staples in our medicine cabinet are made up of chemical substances. These chemicals are made up of a fixed proportion of atoms, and these atoms are arranged in a certain way. In order to figure out what these proportions are and how they are arranged for any given substance, we need to know the chemical formula of the substance or compound.

A compound is a substance made up of a definite proportion of two or more elements. A chemical formula tells us the number of atoms of each element in a compound. It contains the symbols of the atoms of the elements present in the compound as well as how many there are for each element in the form of subscripts.

Each chemical substance has a specific chemical composition, so these chemical substances have their own chemical formula. Let's take a look at the chemical formula of glucose: there are 12 carbon (C) atoms, 22 hydrogen (H) atoms and 11 oxygen (O) atoms.

There are different types of chemical formulas and each type gives us different information about a chemical substance. The different types of chemical formulas include: molecular, empirical, structural and condensed structural formulas. We'll discuss each of these different types as well as go over a few examples.

Molecular Formula

The molecular formula, sometimes known as the true formula, tells us the actual number of the different elements in one molecule of a compound. In a molecular formula, each element is written as their symbols in the periodic table, and the number of atoms for each element is shown by the subscript (the small number to the lower right of the element). Here are some examples of molecular formulas:

If we look at butane, we see it has 4 carbon (C) atoms and 10 hydrogen (H) atoms.

Empirical Formula

The word empirical is defined as something that is verified by observation. In chemistry, we verify facts by performing experiments. So, the empirical formula is defined as the simplest ratio of whole numbers of elements that make up a compound, and this type of formula is derived from experimental data.

Just like how we simplify fractions in math class, in chemistry we can simplify formulas as well. In this case, let's look at the molecular formula of glucose:

While the molecular formula gives us the actual number of atoms of each element in a molecule, the empirical formula gives us the simplest ratio and not the actual number of atoms of an element. Here are some examples of empirical formulas derived from molecular formulas:

Sometimes, there are molecular formulas that are already at their simplest ratio which means they cannot be further reduced. In these cases, the molecular formula is the same as the empirical formula which can be seen with these examples.

In Sucrose, the subscripts 12, 22 and 11 do not have a greatest common factor, so they cannot be further reduced. The same goes with ethanol.

Structural Formula

When we simply write the molecular formula, we do not know how the atoms are arranged or which atoms are bonded to each other. The structural formula shows both the actual number of atoms of elements in a compound, how the atoms are arranged and which atoms are bonded to one another.

Here are the structural formulas of ethane, propane and ethanol. The molecular formulas of each are reflected below the structural formulas.

Let's look at ethane. It shows that the carbon (C) atom on the left is bonded to three hydrogen (H) atoms and the other carbon atom. The carbon on the right is also bonded to three hydrogen atoms and the carbon on the left.

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what is a chemical formula? - definition

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types & examples - video & lesson transcript | study.com

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What is a Chemical Formula? - Definition, Types & Examples - Video & Lesson Transcript | Study.com

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We encounter chemical substances and compounds everyday. The substances under the kitchen sink that we use to clean our houses as well as those that are staples in our medicine cabinet are made up of chemical substances. These chemicals are made up of a fixed proportion of atoms, and these atoms are arranged in a certain way.

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To complete a compound formula, you first need a subscript. A subscript is a small number below and to the right of an atom. The number represents how many of that atom are connected in a molecule. The next thing you need is a Coefficient. A Coefficient is the large number in front of an atom or molecule. It also tells you the number of copies it contains. Every atom alone or combined in a molecule has only one capitol letter for example Ca.

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Identifying Protons, Electrons, and Neutrons

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Identifying Protons, Electrons, and Neutrons

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Mass Number: The mass number is the total number of protons and neutrons in the nucleus of the atom. It is not represented on the periodic table

Atomic Mass: The Atomic Mass is the average of the mass number of all isotopes.

Atomic Number: The Atomic Number is the number of protons an element has. If an element is neutral, then the Atomic Number also can tell you how many electrons there are as well.

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The arrangement of atoms are determined by their physical and chemical properties.

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The relative mass of an electron is 0 because the absolute mass is very small compared to the absolute mass of both protons and neutrons.

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Atoms make up everything around us and make up matter.

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Rutherford had an experiment that used gold foil to discover positive charged particles. To do this he shot alfoparticles at a piece of gold foil. Most of them went right through without being deflected and others scattered and came back.The results of this experiment was the discovery of the nucleus.

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The History of Atomic Chemistry: Crash Course Chemistry #37

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JJ Thomson used a cathodray tube that had both positive and negative electros on each side, and a current run right between the tube. The results of his experiment led to particles that were negatively charged, later known has electrons. JJ Thomson's experiment was named the Plum Pudding Model, with the electrons representing as the plums.

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In his experiment, Dalton discovered that different substances can be made  with the exact same reactants that were used before.

Other Results
-Law of Conservation
Mass of the reactants should equal to the mass of the products.
-Law of Multiple Proportions
If you use the same substance the number that it is divisible by has to be the same.

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1. Atoms cannot be created or destroyed in a chemical reaction
2. All elements are composed of atoms
3. Compounds are composed of different elements.
4. Atoms of different elements are different
5. Atoms of the same element are identical.

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There were 3 scientists who contributed to the development of the atom