Chem 300 Final Exam Study Guide Fall 2017

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Attached. please i need someone to answer these question as sample of final exam . I need someone who is very good in chemstry to answer these and if a question needs an example will be able to explain it well to me

Chem 300 Final Exam Study Guide Fall 2017 Multiple Choice (should take 30s or less to answer) • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • Significant figures (ex. Round to 5 significant figures) Significant figures calculations (adding/subtracting/multiplying/dividing) Scientific notation Converting between metric-to-metric (Ex. Grams to nanograms, etc.) Uncertainty with different types of balances/glassware (Ex. What has the least uncertainty a +/0.1 g balance versus 0.02 g balance) Density (know definition and be able compare to what would be more or less dense) From labs with reading rulers: know how to read a rule to the correct precision and to know the uncertainty. Terms for changes of state (ex. Solid to liquid, etc.) Know diatomic molecules Know group names in periodic table (ex. Noble gases, halogens, etc) For states of matter know properties (ex. Solids – does it have definite volume, shape and what is its kinetic energy like) Definition of a solution Definition of elements, compounds pure substances, homogeneous and heterogeneous mixtures Definition of chemical property and physical property and are they similar/different down a group? Recognize covalent vs. ionic bonds Isotopes – know the definition and be able to determine a neutral and ionized atom when given, protons, neutrons and electrons. Mass number versus atomic number If given a shell how many orbitals and electrons are in the shell. Identify the s block, p block, d block and f block Definition of metals and nonmetals Ionic versus covalent compounds (what is the smallest particle called) Identify valence electrons Chemical change versus physical change Single displacement reactions Be able to identify a decomposition, redox, synthesis/combination, combustion, precipitation, neutralization reaction. Electron configuration for a neutral transition metal and a charged transition metal Definition of dynamic equilibrium Kinetic energy of molecules when gas is cooled Solutions and conductivity. What is a good conductor? Strongly or Slightly ionized solutions? Identify Bronsted-Lowry acids/bases and Arrhenius acids/bases • • • • • Identify strong acids/weak acids and bases If [H+] > [OH-] (or < or =) and compare which would be more acidic, basic or neutral Write the conjugate acid or base Hydrogen atom and electron transition – what transition gives the longest wavelength? The shortest wavelength? Identify what species is oxidized, reduced, oxidizing agent and reducing agent Identify isoelectronic species by looking at electron configuration of neutral and charged atoms Identify where metals, nonmetals and metalloids are located in periodic table Titrations: what is equivalence point? Do you need volumetric glassware? Is it used primarly for acid/base reactions? Is the concentration of one species usually known? Is the indicator arbitrarily chosen? Rank various atoms in order of increasing ionization energy • • • • • • • • • • • • • • Multiple choice calculation problems Use pH calculations Mass % Percent yield Percent by mass - of element within compound. Ex. Find mass percent of O in C2H6O6 Identify species reduced, oxidized, reducing agent, oxidizing agent Calculate oxidation number of specific atom within compound (ex. Cr in Cr2O7) Converting moles to grams, grams to grams, grams to molecules, etc. Use gas law formulas Calculate molarity Titration calculation Convert from celcius to K, etc. pH calculations using pH = -log [H+], etc. Metric to Metric conversions (ex. Kg to ng) Dilution calculation • • • • Worked problems • • • • • • • • • Nomenclature (give the name or formula) Perform significant figure calculations (adding, subtracting, multiplying, dividing) Isotope calculation (ex. Determine the percent natural abundances with masses given) Lewis structure, resonance, electron geometry and molecular geometry Complete and balance reactions (Ex. Bromine and Lithium produce Lithium bromide) Complete and balance a combustion reaction Limiting reagent problem finding masses of both products, calculating percent yield Complete and balance nonionized molecular equation, provide total ionic equation (TIE) and net ionic equation (NIE) Solution stoichiometry More practice: A sample of water was taken with a potassium chloride concentration of 2.5 M. What mass of iron (II) chloride can be formed if excess iron (II) nitrate is added to 35.2 mL of the sample from the lake.

Tutor Answer

Aljon2017
School: Carnegie Mellon University

Hello! I completed the study guide that you have. I made it in a way that the concepts are explained already.If there are problems that you want me to solve - especially for the latter part, please send me some problems that I can solve for you to study later on :)

Chem 300
Final Exam Study Guide
Fall 2017
Multiple Choice (should take 30s or less to answer)
Significant figures (ex. Round to 5 significant figures)
Rules of significant figures:
There are three rules on determining how many significant figures are in a number:
1. Non-zero digits are always significant.
2. Any zeros between two significant digits are significant.
3. A final zero or trailing zeros in the decimal portion ONLY are significant.

Significant figures calculations (adding/subtracting/multiplying/dividing)
For addition and subtraction, look at the decimal portion (i.e., to the right of the decimal point) of the
numbers ONLY. Here is what to do
1) Count the number of significant figures in the decimal portion of each number in the problem. (The
digits to the left of the decimal place are not used to determine the number of decimal places in the final
answer.)
2) Add or subtract in the normal fashion.
3) Round the answer to the LEAST number of places in the decimal portion of any number in the
problem.
The following rule applies for multiplication and division
The LEAST number of significant figures in any number of the problem determines the number of
significant figures in the answer.
This means you MUST know how to recognize significant figures in order to use this rule.

Scientific notation
As an example, let us take 5.14 × 105 = 514000.0
Scientific notation consists of a coefficient (here 5.14) multiplied by 10 raised to an exponent (here 5). To
convert to a real number, start with the base and multiply by 5 tens like this: 5.14 × 10 × 10 × 10 × 10 ×
10 = 514000.0. Multiplying by tens is easy: one simply moves the decimal point in the base (5.14) 5
places to the right, adding extra zeroes as needed.

Converting between metric-to-metric (Ex. Grams to nanograms, etc.)

Density (know definition and be able compare to what would be more or less dense)
The density, or more ...

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Anonymous
Wow this is really good.... didn't expect it. Sweet!!!!

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