bohr diagrams for ions. showing protons, neutrons and electron arrangements
TRANSCRIPT
Bohr Diagrams for Ions
Bohr Diagrams for Ions
Showing Protons, Neutrons and Electron
Arrangements
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 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.
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.
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. Electrons in the outermost occupied shell are called valence electrons.
For example, here is the Bohr model for nitrogen, element number 7.
7 p7 n
For example, here is the Bohr model for nitrogen, element number 7.
7 p7 nThe Valence
Shell
For example, here is the Bohr model for nitrogen, element number 7.
7 p7 n
Valence Electron
Valence Electron
ValenceElectron
Valence ElectronValence
Electron
Here is another example, the Bohr model for magnesium, element number 12.
12 p12 n
Here is another example, the Bohr model for magnesium, element number 12.
12 p12 n
The Valence
Shell
Here is another example, the Bohr model for magnesium, element number 12.
12 p12 nValence
electron
Valence
electron
Here are some points to know about cation and anion formation:
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 p4 n
Lithium atom
3 p4 n
Lithium atom
Valenceelectron
3 p4 n
LithiumLithium atom
3 p4 n
LithiumLithium atom
3 p4 n
LithiumLithium atom
3 p4 n
Lithium ion
3 p4 n
LithiumLithium ion
3 p4 n
LithiumLithium ion
3 p4 n
Lithium ion
3 p4 n
Lithium ion
3 p4 n
Lithium ion
+ 3 charge
3 p4 n
Lithium ion
+ 3 charge
–2 charge
3 p4 n
Lithium ion
+ 3 charge
–2 charge
Net charge
3 p4 n
Lithium ion
+ 3 charge
–2 charge
Net charge = 3
3 p4 n
Lithium ion
+ 3 charge
–2 charge
Net charge = 3–2
3 p4 n
Lithium ion
+ 3 charge
–2 charge
Net charge = 3–2 = +1
3 p4 n
Lithium ion
+1 Net charge = 3–2 = +1
3 p4 n
+1
Bohr Model for a Li+ ion
3 p4 n
+1
Bohr Model for a Li+ ion
2 p4 n
Bohr Model for a Neutral He
Atom
Same electron arrangement as
3 p4 n
+1
Bohr Model for a Li+ ion
2 p4 n
Bohr Model for a Neutral He
Atom
Same electron arrangement as
3 p4 n
+1
Bohr Model for a Li+ ion
2 p4 n
Bohr Model for a Neutral He
Atom
Same electron arrangement as
3 p4 n
+1
Bohr Model for a Li+ ion
2 p4 n
Bohr Model for a Neutral He
Atom
Same electron arrangement as
3 p4 n
+1
Bohr Model for a Li+ ion
2 p4 n
Bohr Model for a Neutral He
Atom
Same electron arrangement as
Bohr Model for a Sulphur Atom
16 p16 n
Bohr Model for a Sulphur Atom
16 p16 n
Valence
Shell
Bohr Model for a Sulphur Atom
16 p16 n
Bohr Model for a Sulphur Atom
16 p16 n
16 p16 n
16 p16 n
16 p16 n
16 p16 n
16 p16 n
16 p16 n
16 p16 n
16 p16 n
16 p16 n
16 p16 n 18 e–
16 p16 n 18 e–
16 p+
16 p16 n 18 e–
16 p+
16 p16 n 18 e–
16 p+
–2
16 p16 n 18 e–
16 p+
–2 Net charge
16 p16 n
–2 Net charge
16 p16 n
–2 Net charge
16 p16 n
2–
16 p16 n
2–
Bohr Model for an S2– or sulphide ion
16 p16 n
2–
Bohr Model for an S2– or sulphide ion
16 p16 n
2–
Bohr Model for an S2– or sulphide ion
18 p22 n
Bohr Model for a neutral Argon
Atom
16 p16 n
2–
Bohr Model for an S2– or sulphide ion
18 p22 n
Bohr Model for a neutral Argon
Atom
16 p16 n
2–
Bohr Model for an S2– or sulphide ion
18 p22 n
Bohr Model for a neutral Argon
Atom
STABLE