Binary Ionic Compounds
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Understanding binary ionic compounds can be a struggle to anyone not in the field of chemistry. I hope this slideshow proves helpful to you! With clear text and examples, this slideshow will teach you the basic points of binary ionic compounds.
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Binary Ionic Compounds
- 1. Binary Ionic Compounds A CHEMISTRY PRESENTATION
- 2. What are Binary Ionic Compounds? • binary ionic compounds are composed of two elements – the positive and negative charges must be equal • remember, “bi-” means “two,” so binary ionic compounds are composed of two atoms
- 3. Superscripts vs. Subscripts • remember, there is a BIG difference between a superscript and a subscript – superscripts (the numbers at the top of an element’s symbol) tell us what an atom’s charge is, and the superscript either is positive or negative – subscripts (the numbers at the bottom of an element’s symbol) tell us how many atoms there are of each element in a formula SUPERSCRIPT SUBSCRIPT Br - O2
- 4. How to Form a Binary Ionic Compound 1. look at the elements’ charges 2. balance the charges so that they equal zero EX. Magnesium + Bromine Mg2+ Br - to balance out the charges (because Mg2+ > Br -, and the charges don’t balance out to zero), we have to add another Br - atom Mg2+ + Br - + Br - imagine this as 2 - 1 - 1 = 0, a neutral charge
- 5. A Quick Math Lesson LET’S GO OVER SOME BASIC BUT VERY IMPORTANT MATH: 1. A NEGATIVE TIMES A NEGATIVE = A POSITIVE 2. A NEGATIVE TIMES A POSITIVE = A NEGATIVE 3. IN A MATH PROBLEM, IF THE NEGATIVE NUMBER IS GREATER THAN THE POSITIVE NUMBER, THEIR SUM IS NEGATIVE 4. IF THE POSITIVE NUMBER IS GREATER THAN THE NEGATIVE NUMBER, THEIR SUM IS POSITIVE
- 6. How to Cross-Over Superscripts • when you combine atoms in binary ionic compounds, you can cross-over superscripts EX. Aluminum + Oxygen Al3+ O- Al3+ O2- and Al3+ O2- TAKE THE 3+ AND THE 2 ON THE AL ATOM AND MULTIPLY THEM (2 X 3+ = 6+), THEN THE 3 AND THE 2- ON THE OXYGEN ATOMS (3 X 2- = 6-). THE TWO PRODUCTS, 6- AND 6, BALANCE OUT TO ZERO. THEREFORE, THE FINAL FORMULA IS Al2O3
- 7. References • Modern Chemistry – Holt, Rinehart, and Winston • http://www.cod.edu/people/faculty/jarman/richenda/ 085_materials/chemical%20bonding%20and %20compound%20formation.htm