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SAT Subject Test: Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.

1. Alpha particle
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Largest radioactive particle - decrease atomic number by 2 and the atomic mass by 4 - range of 5 cm in air - high energy and velocity - 100 -000 ionizations per cm
SO4²?
8.3 to 10.0 - colorless to pink

2. Exceptions to the octet rule
Soluble
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
White
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

3. Trigonal planar
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Miscible with water - flammable - used as fuel - poisonous
3 bonding - 120° - sp² hybridization

4. Covalent-network / atomic solids
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Two compound react to form two new compounds
Non-polar if electronegativity difference is between 0 and 0.4 - in polar bonds the atom with more electronegativity has greater pull on electrons. Single bond is a sigma bond - double and triple bonds have one sigma - and the other are pi bonds.

5. Ethanol
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
DG = DH - TDS
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
ClO3?

6. Boiling point elevation formula
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
CO3²?
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
COH functional group - name ends in -al

7. General properties of alloys
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Same formula - different structure
OH functional group - name ends in -ol
Potassium - Calcium - Sodium

8. Chlorofluorocarbons
Pressure of mixture of gases equals some of individual gas pressures.
Solid at room temperature
Purple/pink
Degrade the oxone layer

9. Brass
Classified as strong bases but not very soluble.
Periods 8 and 9 - lanthanides and actinides
Mixture of copper and zinc
CO - produced from incomplete combustion - very toxic

10. Acetate ion
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Purple
C2H3O2?
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

11. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Gas pressure = atm pressure + height of mercury
NH2 - ends in -amide
4 bonding - 109.5° - sp³ hybridization
3 bonding - 120° - sp² hybridization

12. Ester
Photography
Increases left and down
2 bonding - 1 nonbonding
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

13. Cl - Br - and I compounds are...
M1V1 = M2V2
Increase right and up
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Soluble except when containing Ag? - Hg2²? - or Pb²?

14. Name the six strong acids
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
DH = bonds broken - bonds formed
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

15. Sulfate ion
SO4²?
Increase right and up
Solid at room temperature
Yes in thermo - no in electro

16. Formula for calculating enthalpy change with bond energies
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
2 bonding - 180° - sp hybridization
DH = bonds broken - bonds formed
5 bonding - 90° and 120° - sp³d hybridization

17. Color of excited Li+ - Sr2+ - Ca2+
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Red
Gold
Soluble

18. Isoelectronic
Magnesium
Mixture of copper and zinc
Two atoms with the same number of electrons
Soluble except when containing alkaline earth metals

19. What is the second law of thermodynamics?
White
Disordered systems with higher entropies are favored
Yellow
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

20. Properties of acids
1. Water solutions conduct electricity 2. Will react with metals more active than hydrogen to liberate hydrogen. 3. Change litmus to red 4. Phenolphthalein is colorless 5. React with bases to form water and salt 6. React with carbonates to release ca
2nd group - fairly reactive - pastes are used in batteries
1st group - most reactive metal family - react violently with water - create basic solutions
Classified as strong bases but not very soluble.

21. Isotope
Orientation of orbital in space
Same element - different number of neutrons
Oxide that reacts with water to form either an acid or a base
Soluble except when containing alkaline earth metals

22. Alchohols
Moles of solute / kg solvent
Acid to water
OH functional group - name ends in -ol
Lemon yellow

23. Colloid
3 bonding - 1 nonbonding 107°
Emission of electromagnetic energy after beta - positron - or alpha decay
Potassium - Calcium - Sodium
Solution where particles are between 100 and 1000 nm in size—particles this small will not settle.the particles cannot be filtered - but they do scatter light

24. Resonance structures
Largest radioactive particle - decrease atomic number by 2 and the atomic mass by 4 - range of 5 cm in air - high energy and velocity - 100 -000 ionizations per cm
Moles / L
Orientation of orbital in space
Same molecule - different electron pair positions

25. Hydroxyl group
Acid to water
OH - alcohols - name ends in ol
Limited oxygen
Deadly - yellow-green - weapon

26. Molality
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Two atoms with the same number of electrons
Increases left and down
Moles of solute / kg solvent

27. Ionic bond
2 bonding - 1 nonbonding
Increased
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Acid to water

28. What are the factors that affect reaction rate?
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Orange
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Degrade the oxone layer

29. F compounds are...
Soluble except when containing alkaline earth metals
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
V1/T1 = V2/T2

30. Molecular solids
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Extremely slow reactivity
Involves water
Orange

31. When the reaction is exothermic - the entropy is
Yellow to orange
8.3 to 10.0 - colorless to pink
Decreased
Involves water

32. Molarity
Moles / L
PO4³?
Diamond - graphite - amorphous - fullerenes
Insoluble

33. Color of excited Fe3+
PO4³?
8.3 to 10.0 - colorless to pink
Gold
Make up jet fuels and kerosene

34. Noble gases
DG = DH - TDS
Same molecule - different electron pair positions
Extremely slow reactivity
2 bonding - 180° - sp hybridization

35. Compounds with 1-4 carbons
Gases at room temperature - used for fuel
Oxide that reacts with water to form either an acid or a base
Emission of electromagnetic energy after beta - positron - or alpha decay
White

36. Pi bonds
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
NH2 - ends in -amide
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

37. Sulfide color: Sb2S3
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
4.5 to 8.3 - Red to blue
Mixture of silver and copper
Orange

38. Properties of ionic substances

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39. Carbon monoxide
Orange
CO - produced from incomplete combustion - very toxic
Properties of solutions that depend on the number of particles per solvent molecule
NH4?

40. Oxygen gas properties
Mixture of tin - copper - bismuth - and antimony
21% of atmosphere - colorless - odorless - supports combustion reactions
Increases left and down
PV = nRT - R = .0821

41. Hydrogen gas properties
Gases at room temperature - used for fuel
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Glass and plastic
ClO3?

42. Colligative properties
DH = bonds broken - bonds formed
Increase right and up
Degrade the oxone layer
Properties of solutions that depend on the number of particles per solvent molecule

43. Double replacement reaction
Mixture of iron and carbon
Mixture of tin - copper - bismuth - and antimony
Bright yellow
Two compound react to form two new compounds

44. Rare earth elements
Two atoms with the same number of electrons
Periods 8 and 9 - lanthanides and actinides
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
1st group - most reactive metal family - react violently with water - create basic solutions

45. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Orientation of orbital in space
Make up jet fuels and kerosene
Insoluble

46. If G is negative - is the reaction spontaneous?
Non-polar if electronegativity difference is between 0 and 0.4 - in polar bonds the atom with more electronegativity has greater pull on electrons. Single bond is a sigma bond - double and triple bonds have one sigma - and the other are pi bonds.
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Yes
OH functional group - name ends in -ol

47. Oxides are insoluble and when reacted with water..
Do not conduct electricity well
Nonmetal oxides form acids - metal oxides form bases
No
Green

48. Metallic bonds
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Electrons are free to move through metal structure - high conductivity - ductile
NO3?
P1/V1 = P2/V2

49. Combustion reaction
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Soluble
Two reactants combine to form a single product

50. Alkaline earth metals
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
2nd group - fairly reactive - pastes are used in batteries
Yellow
ClO3?