Test your basic knowledge |

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. bronze
Mixture of copper - zinc - and other metals
CO - produced from incomplete combustion - very toxic
1. don't conduct good current 2. many exist as gases at room temp 3. melting points of solid crystals are low 4. large amount of energy needed to decompose
6.0 to 7.6 - yellow to blue

2. If G is positive - is the reaction spontaneous?
White
No
Same molecule - different electron pair positions
OH functional group - name ends in -ol

3. Boiling point elevation formula
Soluble except when containing Ag? - Hg2²? - or Pb²?
Extremely slow reactivity
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
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

4. Nonmetals
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
1. don't conduct good current 2. many exist as gases at room temp 3. melting points of solid crystals are low 4. large amount of energy needed to decompose
Do not conduct electricity well
Involves water

5. How can hydrogen be produced?
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Blue
Mixture of tin - copper - bismuth - and antimony
Miscible with water - flammable - used as fuel - poisonous

6. Color of MnO4? solution
yellow
3 bonding - 120° - sp² hybridization
Acid to water
Purple

7. Supersaturated solution
3.1 - 4.4 - red to yellow
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Yes
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

8. Hydrolysis reaction
Oxide that reacts with water to form either an acid or a base
Involves water
4.5 to 8.3 - Red to blue
7th group - form salts - always exist as diatomic molecules - used in modern lighting

9. amphoteric
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
2 bonding - 1 nonbonding
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Substance can act either as an acid or a base

10. Nitrate ion
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Potassium - Calcium - Sodium
NO3?

11. Gamma decay
Yellow
Same molecule - different electron pair positions
Emission of electromagnetic energy after beta - positron - or alpha decay
No two electrons can have the same set of 4 quantum numbers

12. Hydrofluoric acid is used for
NH2 functional group - name ends in -amide
Gold
Etching glass and frosting lightblubs
Gas pressure = atm pressure + height of mercury

13. 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
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
1. Solids don't conduct good electrical current. 2. Liquid phase are good conductors 3. Relatively high melting and boiling points 4. Do not vaporize readily at room temperature. 5. Brittle / easily broken 6. Soluble in water
NO3?

14. What are the factors that affect reaction rate?
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Moles / L

15. Graham's Law
6.0 to 7.6 - yellow to blue
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

16. What is the equation used for heat transfer problems?
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Black
Q = mcDT
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

17. Properties of molecular crystals and liquids

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

18. Noble gases
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
yellow
Extremely slow reactivity
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

19. What qualifies as a strong base?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Liquid at room temperature - used to make gasoline and solvents

20. Ethanol
Moles / L
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

21. Halogen properties
COH functional group - name ends in -al
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

22. Compounds with 5-10 carbons
Green
Deadly - yellow-green - weapon
Liquid at room temperature - used to make gasoline and solvents
V1/T1 = V2/T2

23. pewter
Light green
Mixture of tin - copper - bismuth - and antimony
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Two compound react to form two new compounds

24. Ammonium Ion
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
CO - produced from incomplete combustion - very toxic
Mixture of iron and carbon
NH4?

25. Chlorine gas
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Deadly - yellow-green - weapon
Photography
COOH functional group - name ends in oic acid

26. Gibb's Free Energy equation
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
DG = DH - TDS
Soluble except when containing Ag? - Hg2²? - or Pb²?
6 bonding - 90° - sp³d2² hybridization

27. When the reaction is exothermic - the entropy is
Purple/pink
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Same element - different number of neutrons
Decreased

28. Tetrahedral
Diamond - graphite - amorphous - fullerenes
A compound breaks into two parts
4 bonding - 109.5° - sp³ hybridization
Covalent

29. Principal quantum number (n)
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Mixture of silver and copper
Bright yellow
Energy level - as it increases electrons are less bound to the nucleus

30. Chlorate ion
2nd group - fairly reactive - pastes are used in batteries
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
ClO3?
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

31. If G is zero - what is happening in the reaction?
7th group - form salts - always exist as diatomic molecules - used in modern lighting
8.3 to 10.0 - colorless to pink
It is at equilibrium
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

32. Carbonate ion
CO3²?
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
4 bonding - 109.5° - sp³ hybridization
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

33. Sulfide color: ZnS
Yellow to orange
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
White
COOH - ends in -oic acid

34. F compounds are...
1st group - most reactive metal family - react violently with water - create basic solutions
Soluble except when containing alkaline earth metals
Bright yellow
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

35. When a reaction is endothermic - the entropy is
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Increased
Energy level - as it increases electrons are less bound to the nucleus
Q = mcDT

36. Formula for calculating enthalpy change with bond energies
Involves water
Soluble except when containing Ag? - Hg2²? - or Pb²?
DH = bonds broken - bonds formed
Degrade the oxone layer

37. List equivalent pressure values for mmHg - torr - atm - and Pa
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
2 bonding - 1 nonbonding

38. Molecular solids
Periods 8 and 9 - lanthanides and actinides
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
COOH functional group - name ends in oic acid
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

39. Examples of strong electrolytes
NH4?
Strong acids - strong bases - soluble salts
Defines shape of orbital
Soluble except when containing alkaline earth metals

40. Methanol
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Miscible with water - flammable - used as fuel - poisonous
PO4³?
NH4?

41. Suspension
Solid at room temperature
Acid to water
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

42. Properties of ionic substances

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

43. Color of excited Ba2+
Light green
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
Mixture of copper and zinc
Purple/pink

44. Ethers
Two reactants combine to form a single product
M1V1 = M2V2
R-O-R functional group - shorter chain ends in oxy - other is ane
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

45. If G is negative - is the reaction spontaneous?
4.184
Soluble except when containing alkaline earth metals
Yes
Energy level - as it increases electrons are less bound to the nucleus

46. Color of excited Na+
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
yellow
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
ClO3?

47. SO4²? compounds are...
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Soluble

48. What kind of bonds generally hold gases together?
Orange
Covalent
Gas pressure = atm pressure - height of mercury
CO - produced from incomplete combustion - very toxic

49. Halogens
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
OH - alcohols - name ends in ol

50. Covalent-network / atomic solids
Black
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite