Bohr Diagrams for Ions

Showing Protons, Neutrons and Electron Arrangements

Ions Ions are formed when neutral atoms lose or gain electrons

Ions are formed when neutral atoms lose or gain electrons and end up with a positive or negative charge.

A few points to remember:

A proton is + and an electron is –

A few points to remember: A proton is + and an electron is – In a neutral atom the # of protons = # of electrons

A few points to remember: A proton is + and an electron is – In a neutral atom the # of protons = # of electrons When atoms form ions, they do so only by losing or gaining electrons.

A few points to remember: A proton is + and an electron is – In a neutral atom the # of protons = # of electrons When atoms form ions, they do so only by losing or gaining electrons. They never change the number of protons.

A few points to remember: A proton is + and an electron is – In a neutral atom the # of protons = # of electrons When atoms form ions, they do so only by losing or gaining electrons. They never change the number of protons. When a neutral atom loses one or more electrons, it gains a + charge, and it called a cation.

A few points to remember: A proton is + and an electron is – In a neutral atom the # of protons = # of electrons When atoms form ions, they do so only by losing or gaining electrons. They never change the number of protons. When a neutral atom loses one or more electrons, it gains a + charge, and it called a cation. When a neutral atom gains one or more electrons, it gains a – charge, and it is called an anion.

When atoms interact with each other, they use only the electrons in the outermost occupied shell.

valence shell The outermost occupied shell is called the valence shell.

When atoms interact with each other, they use only the electrons in the outermost occupied shell. The outermost occupied shell is called the valence shell. valence electrons Electrons in the outermost occupied shell are called valence electrons.

For example, here is the Bohr model for nitrogen, element number 7. 7 p 7 n

For example, here is the Bohr model for nitrogen, element number 7. 7 p 7 n The Valence Shell

For example, here is the Bohr model for nitrogen, element number 7. 7 p 7 n Valence Electron

Here is another example, the Bohr model for magnesium, element number p 12 n

Here is another example, the Bohr model for magnesium, element number p 12 n The Valence Shell

Here is another example, the Bohr model for magnesium, element number p 12 n Valence electron

Here are some points to know about cation and anion formation:

Elements with 1—3 valence electrons tend to lose these electrons and form positive ions, or cations.

Here are some points to know about cation and anion formation: Elements with 1—3 valence electrons tend to lose these electrons and form positive ions, or cations. Elements with 5—7 valence electrons tend to gain electrons in order to fill up their valence shells.

Here are some points to know about cation and anion formation: Elements with 1—3 valence electrons tend to lose these electrons and form positive ions, or cations. Elements with 5—7 valence electrons tend to gain electrons in order to fill up their valence shells. When they gain electrons they form negative ions, or anions.

Let’s do a couple of examples:

3 p 4 n Lithium atom

3 p 4 n Lithium atom Valence electron

3 p 4 n LithiumLithium atom

3 p 4 n LithiumLithium atom

3 p 4 n LithiumLithium atom

3 p 4 n Lithium ion

3 p 4 n Lithium Lithium ion

3 p 4 n Lithium Lithium ion

3 p 4 n Lithium ion

3 p 4 n Lithium ion

3 p 4 n Lithium ion + 3 charge

3 p 4 n Lithium ion + 3 charge –2 charge

3 p 4 n Lithium ion + 3 charge –2 charge Net charge

3 p 4 n Lithium ion + 3 charge –2 charge Net charge = 3

3 p 4 n Lithium ion + 3 charge –2 charge Net charge = 3–2

3 p 4 n Lithium ion + 3 charge –2 charge Net charge = 3–2 = +1

3 p 4 n Lithium ion +1 Net charge = 3–2 = +1

3 p 4 n +1 Bohr Model for a Li + ion

3 p 4 n +1 Bohr Model for a Li + ion 2 p 4 n Bohr Model for a Neutral He Atom Same electron arrangement as

3 p 4 n +1 Bohr Model for a Li + ion 2 p 4 n Bohr Model for a Neutral He Atom Same electron arrangement as

3 p 4 n +1 Bohr Model for a Li + ion 2 p 4 n Bohr Model for a Neutral He Atom Same electron arrangement as

3 p 4 n +1 Bohr Model for a Li + ion 2 p 4 n Bohr Model for a Neutral He Atom Same electron arrangement as

3 p 4 n +1 Bohr Model for a Li + ion 2 p 4 n Bohr Model for a Neutral He Atom Same electron arrangement as

Bohr Model for a Sulphur Atom 16 p 16 n

Bohr Model for a Sulphur Atom 16 p 16 n Valence Shell

Bohr Model for a Sulphur Atom 16 p 16 n

Bohr Model for a Sulphur Atom 16 p 16 n

16 p 16 n

16 p 16 n

16 p 16 n

16 p 16 n

16 p 16 n

16 p 16 n

16 p 16 n

16 p 16 n

16 p 16 n

16 p 16 n 18 e –

16 p 16 n 18 e – 16 p +

16 p 16 n 18 e – 16 p +

16 p 16 n 18 e – 16 p + –2

16 p 16 n 18 e – 16 p + –2 Net charge

16 p 16 n –2 Net charge

16 p 16 n –2 Net charge

16 p 16 n 2–

16 p 16 n 2– Bohr Model for an S 2– or sulphide ion

16 p 16 n 2– Bohr Model for an S 2– or sulphide ion

16 p 16 n 2– Bohr Model for an S 2– or sulphide ion 18 p 22 n Bohr Model for a neutral Argon Atom

16 p 16 n 2– Bohr Model for an S 2– or sulphide ion 18 p 22 n Bohr Model for a neutral Argon Atom

16 p 16 n 2– Bohr Model for an S 2– or sulphide ion 18 p 22 n Bohr Model for a neutral Argon Atom STABLE