combining elements how chemical compounds are made
DESCRIPTION
Metals and Non-metals Metals have a tendency to lose electrons and form positive (+) ions. Non-metals tend to gain electrons and form negative (-) ions Positive and negative charges attract When a positive ion and a negative ion bind together they form an ionic bondTRANSCRIPT
Combining ElementsHow Chemical Compounds Are Made
Combining Elements
• Elements can exist on their own but most matter consists of two or more elements combined together
• How do they combine??
Metals and Non-metals
• Metals have a tendency to lose electrons and form positive (+) ions.
• Non-metals tend to gain electrons and form negative (-) ions
• Positive and negative charges attract• When a positive ion and a negative ion bind
together they form an ionic bond
Example (Sodium and Fluorine)
• An atom of Sodium has a single electron in its outer orbittal. This makes it unstable
• An atom of fluorine has seven electrons in its outer orbital. It needs one more to be stable.
Metal and Non-Metal
• So they make a deal!
• The sodium gives an electron to fluorine
• Now they’re both happy
• The only thing is:– They’re not atoms any more
•They’re IONS• An ion is like an atom but it has a charge
• Now REMEMBER–Opposites attract!
Ionic Compounds
• So sodium and fluorine are attracted to each other and form an inseparable bond
And they call themselves Sodium Fluoride!! (or NaF)
Sodium Fluoride is an Ionic Compound
Ionic Compounds
Here’s another example:• Let’s take Calcium and Chlorine
• Calcium needs to get rid of two electrons to be stable but Chlorine only needs one.
• SO WHAT CAN THEY DO?
Building Ionic Compounds
• What if Chlorine found a friend?
• Another chlorine atom!
Making Ionic Compounds
• Now Calcium can give one electron to each of them!
• Now everyone’s happy!
Making Ionic Compounds
• This compound is called Calcium Chloride• Or CaCl2
• Because there is one calcium ion and two chlorine atoms
Making Ionic Compounds
• Making ionic compounds is easy if you follow a few rules
1. Write down the name (or symbol) of each element starting with the metale.g. Potassium (K) Sulfur (S)
2. Beside each one, write down the number of electrons that the element needs (or has to give away) to be stable
K (1) S (2)3. Now criss cross the numbers
K (1) S (2)
Making Ionic Compounds
• This gives us K2S or Potassium Sulfide• Try these
Metal Non-metal Metal Symbol &
Electrons to lose
Non-metal Element
and Electrons to
gain
Final Formula
(Criss cross)
Magnesium Nitrogen Mg (2) N (3) Mg3N2
Lithium Chlorine
Calcium Carbon
Aluminum Silicon
• One last thing– If you can divide both numbers by a highest common
factor: DO IT!!
–Example: Calcium OxideCa2O4
• 2 and 4 are both divisible by 2 so• Ca2O4 becomes CaO2
Naming Binary Ionic Compounds
• A binary ionic compound is an ionic compound with two elements.
• They’re very easy to name.1. Write down the metal first, then the non-metal.2. The metal keeps its name. 3. Now take the non-metal, write down its first
syllable and then write ide. 4. That’s it! You’re done!
Naming Binary Ionic Compounds• Example
•Mg3P2
•Magnesium PhosphideNow try these
Formula NameNa2OAlCl3
Be3S2
More PracticeTry these (Name Formula)
Compound Symbols and “Criss-Cross”
Formula
Calcium Chloride
Beryllium Phosphide
Aluminum Oxide
Potassium Nitride
Magnesium Carbide
Sodium Iodide
Lithium Sulfide
Now Try These (Formula Name)
Formula NameCaF2
Al4Si3
Mg3P2
BeI2
LiFCa2CNa3P