Chemistry- Formulas

emilybaitman
Note by emilybaitman, updated more than 1 year ago
emilybaitman
Created by emilybaitman over 6 years ago
25
2

Description

Note on Chemistry- Formulas, created by emilybaitman on 04/12/2014.

Resource summary

Page 1

Isotopes- Atoms of the same element with a different number of neutrons

Relative Formula Mass (Mr)-Example-Find the Mr of carbon monoxide- COCarbon= 12 Oxygen=1612+16=28Find the Mr of sodium oxide- Na2OSodium= 23 Oxygen= 16(23x2)+16=62Moles-one moleof that substance. For example, the Mr of carbon monoxide (CO) is 28. This means that one mole of carbon monoxide has a mass of 28 g. You should be able to see that: 14 g of carbon monoxide contains 14 ÷ 28 = 0.5 moles 56 g of carbon monoxide contains 56 ÷ 28 = 2 moles

Empirical Formula-Question- 3.2g of sulfur reacts with oxygen to produce 6.4g of sulfur oxide.Use the fact that Ar of sulfur is 32 and Ar of oxygen is 16.Answer- find the mass of each of the elements first.Oxygen= 6.4-3.2=3.2Now divide each of the elements mass by its Ar value.Sulfur: 3.2/32=0.1Oxygen: 3.2/16=0.2Fine the ratios of the elements, you can do this by dividing the smallest of the numbers to give you the number of atoms of each element in the compound.Sulfur: 0.1/0.1=1Oxygen: 0.2/0.1=2(if one of these number ever ends in .5 then multiply both numbers by 2)So this tells us that there is one sulfur and two oxygen's so the formula is SO2

New Page

Show full summary Hide full summary

Similar

Ch. 2: The Chemical Context of Life Notes
Emma Cress
The Nature of Matter
Billy White
Elements of Life
Nathan Butler
Chapter 1
Bethany Westwood
Chemistry Review
Urvee ___
Atomic Mass Quiz
Holly Nephew
Atomic Mass
Holly Nephew
Intro to Geology
Chika Abigail
C2 bonding
chapel.jacquesel
Modern Atomic Model 2
Niamh Ryan
Average Atomic Mass
Holly Nephew