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  • For example, you could run the command atom./hopes./dreams to open both the hopes and the dreams directories at the same time. When you open Atom with one or more directories, you will automatically get a Tree View on the side of your window. The Tree View allows you to explore and modify the file and directory structure of your project.
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  1. Atom Examples In Real Life
  2. Atom Definition Chemistry
  3. Edible Atom Examples
  4. Atom Example Sentence

An ion is an atom or group of atoms where the number of electrons is not equal to the number of protons. Electrons have a negative charge, whereas protons have a positive charge. When an atom gains electrons, this results in a negative charge. This type of ion is called an anion. When an atom loses electrons, this results in a positive charge. A positively charged ion is called a cation. Let's explore several ion examples of both types.

Examples of Positive Ions

Positive ions are typically metals or act like metals. Many common materials contain these ions. Mercury is found in thermometers, for instance, and aluminum is a metal that is found in a surprising amount of things. It's even an ingredient in baking soda and in certain other food products!

For example, H2O consists of an Oxygen atom linked to 2 Hydrogen atoms. The linkage or interaction between the electrons of the Hydrogen and Oxygen atoms is called a Chemical Bond. More on these later. Atoms in the Human Body. The human body is made up of a couple dollars worth of chemicals.

The positive charge (more protons versus electrons) for a cation is shown by a number and plus sign after the formula. If there's just a plus sign, it means the charge is plus 1. Some examples of cations, or positive ions, include the following:

  • Aluminum - Al+3
  • Barium - Ba+2
  • Bismuth - Bi+3
  • Cadmium - Cd+2
  • Calcium - Ca+2
  • Cesium - Cs+
  • Chromium (III) - Cr+3
  • Cobalt - Co+2
  • Copper (I) - Cu+
  • Copper (II) - Cu+2
  • Hydrogen - H+
  • Iron (II) - Fe+2
  • Iron (III) - Fe+3
  • Lead (II) - Pb+2
  • Lithium - Li+
  • Magnesium - Mg+2
  • Mercury (I) - Hg2+2
  • Mercury (II) - Hg+2
  • Nickel - Ni+2
  • Potassium - K+
  • Rubidium - Rb+
  • Silver - Ag+
  • Sodium - Na+
  • Strontium - Sr+2
  • Tin (II) - Sn+2
  • Zinc - Zn+2

Examples of Negative Ions

Just as atoms can lose electrons to become cations, some can gain electrons and become negatively charged anions. Again, you may be familiar with some of these ions. Fluoride is sometimes added to community water supplies. Your dentist may also give you a flouride treatment.

The negative charge (fewer protons than electrons) for an anion is shown by a number and minus sign after the formula. If there's just a minus sign, it means the charge is minus 1. Here are several examples of anions:

Atom
  • Bromide - Br-
  • Chloride - Cl-
  • Fluoride - F-
  • Iodide - I-
  • Nitride - N3-
  • Oxide - O2-
  • Sulfide - S2-

Polyatomic Cations and Anions

If an ion consists of two or more atoms it is called a polyatomic ion. Just like their single-atom counterparts, they too can gain and lose electrons.

Polyatomic Cations

Ions with multiple atoms that lose electrons, and are thus positively charged, are called polyatomic cations.

  • Ammonium - NH+4
  • Hydronium - H3O+

Polyatomic Anions

Ions with multiple atoms that gain electrons, and are thus negatively charged, are called polyatomic anions. In the list below, the charge has been put in parentheses for ease of legibility, but standard notation calls for the charge to be written as a superscript instead.

  • Acetate - CH3COO- or C2H3O2-
  • Arsenate - AsO43-
  • Bicarbonate or hydrogen carbonate - HCO3-
  • Borate - BO33-
  • Carbonate - CO32-
  • Chlorate - ClO3-
  • Chlorite - ClO2-
  • Chromate - CrO42-
  • Cyanide CN-
  • Dichromate - Cr2O72-
  • Dihydrogen phosphate - H2PO4- or H2O4P-
  • Formate - CHO2- or HCOO- or CHOO-
  • Hydrogen sulfate or bisulfate - HSO4-
  • Hydrogen sulfite or bisulfite - HSO3-
  • Hydrogen phosphate - HPO42-
  • Hydroxide OH-
  • Hypochlorite - ClO-
  • Nitrate - NO3-
  • Nitrite - NO2-
  • Oxalate - C2O42-
  • Perchlorate - ClO4-
  • Permanganate - MnO4-
  • Peroxide O22-
  • Phosphate - PO43-
  • Phosphite - PO33-
  • Silicate - SiO32-
  • Sulfate - SO42-
  • Sulfite - SO32-
  • Thiocyanate - SCN-
  • Thiosulfate - S2O32-

Ionic Compounds

Examples

Atom Examples In Real Life

An ionic compound is made up of one or more anions and one or more cations.

Atom Definition Chemistry

Some examples of ionic compounds include:

  • Aluminum sulfide - Al2S3
  • Beryllium chloride - BeCl2
  • Boron iodide - BI3
  • Calcium nitride - Ca3N2
  • Copper phosphide - Cu3P
  • Iron (II) iodide - FeI2
  • Iron (III) oxide - Fe2O3
  • Lead (II) sulfide - PbS
  • Lead (IV) phosphide - Pb3P4
  • Lithium fluoride - LiF
  • Magnesium chloride - MgCl2
  • Potassium bromide - KBr
  • Sodium fluoride - NaF
  • Sodium nitride - Na3N
Atom Examples

Fully Charged Reaction

Edible Atom Examples

When you study chemistry, you will encounter many examples of ions, as well as the different types of ions and how they interact and relate to each other. For more on the topic, be sure to explore some examples of chemical bonds and examples of chemical properties. Perhaps they'll be the catalyst for positive change in your learning experience!

Atom Example Sentence

Atoms in everyday life

So now you know the definition of an atom...but that's far from having knowledge of an atom! Atoms are extremely important structures that make up all of the materials on earth. Atoms are in our bodies and they bond together to form molecules, which make up matter.
Matter is any substance that takes up space, meaning it has mass and volume. The three main forms of matter are solid, liquid, or gas.
The Atomic Theory
In the history of atoms we will go more in depth about Dalton's atomic theory. But as an introduction, the Atomic Theory was a theory that justified the idea that all matter is made up of atoms. This means that mostly anything in the world is made up of atoms.
Atomic Bonding
In order to create the matter that exists on the earth, atoms must be held together by something. The atraction that keeps atoms bonded to each other is called chemical bonding.Chemical bonding keeps atoms together by the postive charge from one atom and the negative charge from another forcing together. The positive charge comes from the nucleus of an atom and the negative charge comes from the electron cloud of another atom. The bond of two atoms isn't the atoms themselves, but the force between them. The four main, most common types of bonding are molecular covalent, network covalent, ionic, and metallic.
Covalent Bonding: Covalent bonds occur when atoms bond together by sharing electrons. The two types of covalent bonding are
Molecular Covalent: These bonds are created by nonmetal atoms and they are either gases or liquids. Molecular covalent bonding occurs when atoms share valence eltectrons between each other. As a ressult of sharing valence electrons, a molecule is created. These types of bonds do not conduct electricity, and they may or may not dissolve in water.
Network Covalent:These bonds are created by nonmetal atoms just like molecular covalent bonding, but they are made of solids. Instead of the valence electrons being shared between the atoms, in network covalent bonding the electrons are shared amongst the entire atoms. These types of bonds do not conduct electricity, nor do they dissolve in water.
Ionic Bonding:Ionic bonds are metal and nonmetal atoms joined together and they form solids. Ionic bonding occurs when the
nonmetal atom receives valence electrons from the metal atom due to the transportation of valence electrons. Ionic bonds dissolve in
water, and once dissolved they can conduct electricity.
Metallic Bonding: Metallic bonds are created by metal atoms and they form solids. Metallic bonds occur when valence electrons
have the ability to move around the atoms and the bond. Metallic bonds can conduct electricity, but they cannot dissolve in water.
The Importance of Atoms
In the most simple terms, without atoms there would not be a functioning world. Atoms make up matter, and matter makes up everything in the world, with a few exceptions. Here are some examples of how atoms affect the world:
-Oxygen atoms are in the air and keep up alive because we need oxygen in order to breathe
-Carbon dioxide atoms are released from our bodies and plants take in the CO2 so that they can photosynthesize
-Hydrogen atoms and oxygen atoms bond togther to form H2O which is water. Water is so important in the world because it has a
multitide of uses (drinking, cleaning, cooking, transportation). Without water we would not survive.
-Lead atoms bond together and they make up the lead that we use as a pencil.
-Copper atoms, aluminum atoms, nickel atoms, etc., all make up metal which is used for a variety of things in everyday life.