Upload
elwin-spencer
View
220
Download
4
Embed Size (px)
Citation preview
Subatomic Particles (Table 2.1)
Particle Mass
(g) Relative
Mass (amu) Charge
Electron (e-) 9.1 x 10-28 0 -1
Proton (p+) 1.67 x 10-24 1 +1
Neutron (n0) 1.67 x 10-24 1 0
++
++
+
the particlesthat make up atomshave eitherpositive or negative charge
In order to understandwhat ions are,we need to know that…
++
++
+
Positive and negative are opposites
they cancel each other out
Therefore, the net charge = zero
++
++
+
In an atom,protons ( ) are inthe centerand electrons ( )are on the outside
+
only electrons ( )can be addedor taken away
++
++
+
This is an atom with5 electrons and
5 protons
the atom is neutral net charge = zero
Equal “+” and
“-” charges
WHEN REMOVING ELECTRONS
THE RESULTING CHARGE IS POSITIVE
neutral 1+
We are now LESS negative = MORE positive
THE RESULTING CHARGE IS NEGATIVE
neutral 2
WHEN ADDING ELECTRONS
We are now MORE negative = LESS positive
Notice that ONLY the number of e- changes
The number of protons in anAtom NEVER changes –
They are trapped inside the nucleus
(Only electrons are added or subtracted)
An ion is an atom, or group of atoms, that has a net positive or negative charge.
cation ion with a positive charge. If a neutral atom loses one or more electrons it becomes a cation.
anion ion with a negative charge. If a neutral atom gains one or more electrons it becomes an anion.
Na 11 protons11 electrons Na+ 11 protons
10 electrons
Cl 17 protons17 electrons Cl- 17 protons
18 electrons
How do we know what charge our ion will
have????
We need to look at our Bohr-Rutherford Diagrams
-Most atoms on their own will form ions to complete their outer orbit (energy level)
Put simply - An atom wants to have a full outer orbit (2 for He, 8 for others). To do this they can either:-Lose 1 or more electrons (cation +)
-Loses outer orbit
Or
-Gain 1 or more electrons (anion -)-Fills outer orbit
How do you know which it will be?
It will be whatever is easier
-If it has 1 valence electron it will lose 1 and lose its outer orbit easier to lose 1 than gain 7
- If it has 7 valence electrons it will gain 1 to get 8 easier to gain 1 then lose 7!
IonsWe will only be dealing with groups:
1, 2, 13, 15, 16, 17
**Generally speaking, elements on the left (metals and metalloids) will lose e’ to form cations while elements on the right (non-metals) will gain e’ to form anions **
The shortcut!-Look at your periodic table-Ignore the transition metals, the carbon family and Boron-Overtop of the groups write how many electrons they will lose or gain to have a complete outer orbit 8 (or 2 for H and He)-Write whether it will lose the electrons (+) or gain (-)
**Remember, gaining electrons gives a “-” charge**-Example, Be – will lose two to shed its outer orbit = Be+2+
1+2
+3
-3 -2 -1
10 n0
How to properly draw ions
-• Draw Bohr-Rutherford Diagram• Include protons and neutrons in nucleus• Put square brackets around diagram• Place charge top right
Naming IonsPositive Ions – The name is the same as the name of the element followed by ione.g. Na+ = Sodium Ion
Negative Ions – The name is determined by removing the end and adding idee.g. Oxygen Ion = Oxide ion, Phosphorus Ion = Phosphide ion
Multivalent Ions
-Mostly involves transition metals (Copper, Iron) but also includes Tin (Sn) as well as a few others
-Multiple charges are possible therefore you need more information
Multivalent Ions – Write the name given the symbol
Multivalent Ions – Write the name and Roman Numerals-If you are given the Symbol with the charge you can write the name but you must include the roman numeral which represents the charge - E.g. Cu4+ = Copper (IV) ion- Ni3+ = Nickel (III) ion
-** I=1, II=2, III=3, IV=4, V=5, VI=6, VII=7
Multivalent Ions – Write the Symbol given the name
-The Roman Numeral in the name represents the charge on the ion
-E.g. Lead (IV) ion = Pb4+
-Cobalt (II) ion= Co2+
-**Multivalent Ions will always be positive because they are metals