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*Unit 8 Topics
Aldehydes and Ketones
Alkenes and Alkynes
Amines and Amides
An overview of molarity problem
Atomic Mass and Avogadro's Hypothesis
atomic number and mass
Balancing Chemical Reaction Equations
Basic Science definitions.
Calculations involving the Mole and the Mass of a Substance and the Volume of a gas
Calculations involving the Mole and the Volume of a gas and the Number of Particles
Certain & Uncertain Digits, Defined Numbers and Accuracy & Precision
Chemical Equations and the Conservation Laws
Chemical families -- by Judy Bai
Classification of matter
Concentration of ions in Solution
Constructing the name of an Ionic Compound
Derived Quantities and Density
Early atomic models
Electrostatic forces, electron shells, Valence electrons and valence of an atom
Energy Changes in Chemical Reactions
Ethers and Carboxylic Acids
History of the period table
How to Classify Atoms and Ions
How to Read a Scale
INTERMOLECULAR FORCES AND BONDING
Introduction to functional groups and Alcohols---Elizabeth
Introduction to organic chemistry and hydrocarbon
Ionization energy, Electron Affinity, Atomic Radius
Isotopes and their mixtures
Lab safety 2
Later atomic models
Lewis Dot Diagrams of Neutral Atoms, Monatomic Ions,and Ionic Compounds
LIine spectra, electron shells and energy level diagrams
Mixing Two Solutions and Making Dilute Solutions
Molar Concentrations and Making up Solutions
Multiple conversions between moles,mass, volume and number of particles
Multiplying & Dividing and Adding and Subtracting with Sig Figs
Naming Hydrates and Naming Compounds Using the Prefix System
Naming Monatomic and Polyatomic Ions
Percent Yield and Purity
Phase Changes--by AnnYU
Phases, the Magic 7 and Chemical Word Equation
polar and nonpolar solvents
SI Units and Metric Unit conversions
Significant Figures & Zeros
Solutions and Solubility Introduction
Solving Problems that Involve Multiple Operations and Sig Figs
Stoichiometery calculation involvingMoles, Mass, Gas volume and Molecules
Stoichiometry Calculations Involving Molar Concentration
Stoichiometry of Excess Quantities
The Conductivity of Aqueous solutions
The Major divisions of the periodic table & Metals Non-metals and semi conductors
The Meaning of Stoichiometry and the Coefficients in a Reaction Equation
The Mole Concept and Finding Molar Mass
The nature of covalenting bonding & Predicting the formula of covalent bonds
The nature of solutions of ions
The Physical separation of substances
THE PHYSICCAL PROPERTIES OF MATTER
The role of Kinetic Energy in Phase Changes
TO DRAW A Lewis dot diagrams of covalent compounds
Types of Chemical Reactions - Combustion (Pt.2) &Summary
Types of Chemical Reactions - First 4 Types
Unbranched Alkanes and their Geometry
When to use each separation method
Writing electron configurations of atoms in full and core notation
Writing electron configurations of ions, and the copper and chromium exceptions
Derived Quantities and Density
Derived Quantities and Density (Page23--26)
: We need to identify what derived quantities are.
The reason why density is considered as derived quantities.
Getting to know some other examples of derived quantities.
derived quantity, derived unit, mass, density
To begin with, a
derived quantity means the combination of other quantities
For instance, density is a derived quantity because is determined by using the mass and the volume of an object.
Density = mass per unit volume or Density = mass / volume
If mass is in g and volume is in mL,
for example, then the unit for density will be in
Here is an example problem: If a 5.0 mL (or 5.0 cm
) piece of copper has a mass of 44.6 g, calculate the density of copper. d = mass / volume d = 44.6 g / 5.0 mL = 8.9 g/mL
: both mass and volume can be directly measured, but density is calculated using two known quantities (
d = m / V
), so density is a derived quantity.
Another derived quantity could be speed, as it is calculated using distance and time. v = d / t, where v is the speed, d is the distance (or displacement), and t is the time. Quantities like mass, length, temperature, etc. can be measured directly and are not determined using other quantities, so they are not "derived" quantities.
Quantities like mass, length, temperature, etc. can be measured directly and are not determined using other quantities. Like mass can be measured by balance, while length and temperature can be calculated by ruler and thermometer. Thus, they are not consider as "derived" quantities
In table1,they are not consider as derived quantities because they can be measured by some tools.
In table2, all of them are consider as derived quantities because these quantities cannot be directly by some tools. While, they need to combine some quantities in order to get the results.
Some practice problem:
1.An iron bar has a mass of 125g. If iron's density is 7.86 x 10
g/L, What volume does the bar occupy?
2.If the density of copper is 8.92 x 10
g/L and the densiy of magnesium is 1.74 x 10
g/L, what mass of magnesium occupies the same volume as 100.0 g of copper?
Do these two practice problems by yourself to test whether you understand the material or not~
Here is the answer key for practice problems above:
1.V=m/d =125g/7.86 x 10
g/L=0.01121 L=volume of magnesium
mass of magnesium=d x V=1.74 x10
g/L x0.01121=19.5g of magnesium
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