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36 Cards in this Set

  • Front
  • Back
What physical properties make the techniques below possible?
1. Settling/Centrifuge
2. Distillation
3. Filtration
1. Density
2. Boiling Point
3. Size of Particles
Define chemical and physical changes.
A chemical change is when new bonds are broken or formed to create a new substance. A physical change is when just an exterior appearance changes, such as color.
Define accuracy and precision.
Accuracy is how close something is to its actual value (the average) and precision is if the measurements are all in the same area, but may not be close to the actual value.
Convert the following from standard notation to scientific.
1. 0.0004550
2. 1000400.0
1. 4.55 x 10 ^ -4
2. 1.0004 x 10 ^ 6
Convert the following.
1. 0.0034 km to cm
2. 455 mm to m
1. 340 cm
2. .455 m
Convert 2 cL to 4 teaspoons.

(1 teaspoon = 5 mL, 1 tablespoon = 3 teaspoons)
4 teaspoons
Calculate the % mass pf water if somebody weighs 145 lbs., 30 of which is water.
20.69 % water
Density of zinc is 7.14 g/mL. If you have 0.5 kg zinc, how many L of zinc do you have?
0.07 L zinc
Write out the actual name (including roman numerals) for 1. Fe2 03
2. Al PO4
1. Iron (II) Oxide
2. Aluminum Phosphate
COmplete the following with the given information.
Formula MM G Particles Moles
1. Ca(OH)2 0.034
2. C6 H5 OH 0.5
1. mm= 74.08 particles= 2.76 x 10 ^ 20 moles= 0.000458

2. mm= 94 grams= 47 particles= 3.01 x 10 ^ 23
Find the empirical formula of
1. C2 H6
2. C5 H15 O10
1. C H3
2. C H3 O2
Find the empirical formula of the compound:
C: 19.78%
O: 43.96%
H: 5.49%
N: 30.77%
C3 O5 H10 N4
If the molar mass to C3 O5 H10 N4 is 546, then what is the molecular formula?
C9 O15 H10 N12
Translate into words:
Cr Cl3(aq)+ 3Na(s) => 3Na(aq) + Cr(s)
Aqueous chromium chloride and solid sodium yield aqueous sodium chloride and solid chromium
Mg3 N2 + 6H2 O => 3Mg (OH)2 + 2NH3
1. If 6.5 mol H2 O react, how many moles of NH3 will form?
2. If you mix together 233g Mg3 N2 and 55g H2 O, what is the limiting reagent?
1. 2.16 mol NH3
2. H2 O is the limiting reagent
Classify the reactions, predict the products and balance the equations.
1. Mg + HCl =>
2. N2 O5 =>
1. Single replacement, becomes 2Mg + 2HCl => 2MgCl + H2
2. Decomposition, becomes 2N2 O5 => 4N + 5O2
Draw the fololwing atomic models.
1. Dalton/Proust
2. Thomson
3. Rutherford
1. Just a circle with a neutral inside.
2. "Plum pudding model", large + center with many - around it.
3. Smaller + center ith many - around it.
4. Small + center with many - rotating or orbiting around on circles.
Rank the following type of electromagnetic waves in terms of energy.

x-ray, visible, gamma, radio, microwaves, ultraviolet and infrared
G, X, UV, V, I, M, R
Wat is the most common isotope for...
1. Ar
2. U
1. 40
2. 238
Name the energy levels colors in order from greatest transition (fall) to the smallest. (6 colors from red to purple)
P, B, G, Y, O, R
Fill in the missing information:
A # # N # E Atomic Mass
28 Ni
(given the charge is +2)
Atomic #= 28, # Neutrons= 29, # Electrons= 26 and Atomic Mass= 57
Complete the equations:
1. U-238 undergoes alpha decay
2. C-14 undergoes beta decay
1. 238 4 242
92 U => 2 He + 94 Pu
2. 14 0 14
6 C => -1 e + 7 N
Describe the charge, mass and what it is stopped by for
1. Alpha
2. Beta
3. Gamma
1. +2, 4, paper
2. -1, 0, wood
3. 0, 0, lead
You have 30g of element Z, which hasa half-life of 3 hours. How much of element Z did you have 15 hours ago?
960g 15 hours ago
List all of the subshells from lowest to highest energy.
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d
1. Write the long form for electron configuration of Ti +.
2. Write the condensed form of Es.
1. 1s2 2s2 2p6 3s2 3p6 4s2 3d1
2. [Rn] 7s2 5f10
Show the trends for Zeff, Ionization Energy, Reactivity and Atomic Radius.
The rend for Zeff is it grows from left to right, Ionization Energy grows from left to right and up, Reactivity grows for gases from left to right and up and for metals grows right to left and down, and Atomic Radius grows from right to left and down.
Calculate the Zeff for
1. B
2. Zn
Zeff is found by Total Protons - Core Protons to get the number of valence electrons, or the Zeff.
1. 3
2. 2
Use electronegativity values to classify the following bonds as ionic, covalent or polar covalent.
1. H-Cl
2. K-Cl
1. 0.96, Polar
2. 2.34, Ionic
Draw Lewis structures for
1. CH3 CH2 CO2-
2. C2 H3 Cl
1. O H H
with one double bond between the C-O, resonance for that double bond.
2. H H
H C C Cl
with one double bond between the C-C.
Circle the following with stronger IMFs and say why.
1. C2 H4 or C3 H4
2. CH4 or CH3 Cl
1. C3 H4 because both have the same electronegativity, but C3 H4 has more electrons.
2. CH3 Cl because it is dipole-dipole due to the electronegativity values between H-Cl.
Answer if the following increases or decreases due to stronger IMFs.
1. boiling point
2. volatility
3. viscosity
4. surface tension
1. increases
2. decreases
3. increases
4. increases
1. My parts are arranged in a crystal lattice. What kind of solid am I and when am I a good conductor of electricity?
2. I am a good conductor of electricity as a solid. What kind of solid am I and do I have a high or low melting point?
1. Ionic solid, poor conductor as a solid, good as a liquid or dissolved in water.
2. Metallic solid, high melting point.
You want to heat 200g of cocoa in a microwave from 25C to 80C. The specific heat of cocoa is 4.18 J/g(K), how many Joules are needed?
q = (200)(4.18)(55)
= 45980 Joules
Use the following information to answer the questions.
Heat of Fusion(Ice) 6.01kJ/mol
Heat Capacity(Water)4.19J/(g(K)
1. How much energy in kJ would it take to melt 50g ice?
2. How much energy in J would it take to heat 50g water from 0 to 100C?
1. (Use heat of fusion)
q = 2.77(6.01)
= 16.65 kJ
2. q = 50(4.19)(100)
= 20950 J
After these flashcards have been completed see the final review packet for the last 10 or so problems.
After these flashcards have been completed see the final review packet for the last 10 or so problems.