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. Hydrofluoric acid is used for
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Etching glass and frosting lightblubs
21% of atmosphere - colorless - odorless - supports combustion reactions

2. Bromthymol blue: pH range and colors
ClO3?
6.0 to 7.6 - yellow to blue
Two compound react to form two new compounds
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

3. Compounds with 18 carbons
Solid at room temperature
It is at equilibrium
Degrade the oxone layer
1st group - most reactive metal family - react violently with water - create basic solutions

4. What is the equation used for heat transfer problems?
Same formula - different structure
Q = mcDT
Insoluble
P1/V1 = P2/V2

5. Silver bromide and silver iodide are used for
ClO3?
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Make up jet fuels and kerosene
Photography

6. Freezing point depression formula
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
DG = DH - TDS
Two atoms with the same number of electrons
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

7. Halogens
7th group - form salts - always exist as diatomic molecules - used in modern lighting
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Spin is +1/2 or -1/2 in an orbital
NH2 functional group - name ends in -amide

8. 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
Blue-green
Purple
NO3?

9. Sulfide color: ZnS
White
yellow
Soluble except when containing alkaline earth metals
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

10. Colligative properties
Properties of solutions that depend on the number of particles per solvent molecule
Moles of solute / kg solvent
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
It is at equilibrium

11. Ketone
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Glass and plastic
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

12. Electronegativity
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Increase right and up
Mixture of copper - zinc - and other metals
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

13. Alpha particle
Increase right and up
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
8.3 to 10.0 - colorless to pink
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

14. What 3 metals will react with cold water?
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
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Potassium - Calcium - Sodium
OH - alcohols - name ends in ol

15. If G is positive - is the reaction spontaneous?
Degrade the oxone layer
Soluble except when containing Ag? - Hg2²? - or Pb²?
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
No

16. What are the allotropic forms of sulfur?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Nonmetal oxides form acids - metal oxides form bases
DH = bonds broken - bonds formed
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

17. Examples of amorphous solids
Diamond - graphite - amorphous - fullerenes
Solid at room temperature
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Glass and plastic

18. Formula for calculating enthalpy change with bond energies
DH = bonds broken - bonds formed
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
White

19. Tetrahedral
Disordered systems with higher entropies are favored
Pressure of mixture of gases equals some of individual gas pressures.
4 bonding - 109.5° - sp³ hybridization
NO3?

20. Hydrogen gas properties
Red
COOH - ends in -oic acid
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

21. Color of Ni2+ solution
Green
Spin is +1/2 or -1/2 in an orbital
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Energy level - as it increases electrons are less bound to the nucleus

22. Octahedral
Oxide that reacts with water to form either an acid or a base
6 bonding - 90° - sp³d2² hybridization
Potassium - Calcium - Sodium
Green

23. Coal
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Substance can act either as an acid or a base
OH - alcohols - name ends in ol
Glass and plastic

24. Isomer
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Properties of solutions that depend on the number of particles per solvent molecule
Same formula - different structure

25. Color of excited Ba2+
NO3?
6.0 to 7.6 - yellow to blue
Mixture of copper and zinc
Light green

26. Compounds with 1-4 carbons
Soluble except when containing Ag? - Hg2²? - or Pb²?
Periods 8 and 9 - lanthanides and actinides
Gases at room temperature - used for fuel
Oxide that reacts with water to form either an acid or a base

27. Charles' Law
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
Gases at room temperature - used for fuel
V1/T1 = V2/T2
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

28. Sulfide color: Sb2S3
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
2nd group - fairly reactive - pastes are used in batteries
Same formula - different structure
Orange

29. Phenolphthalein: pH range and colors
P1/V1 = P2/V2
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
8.3 to 10.0 - colorless to pink
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

30. Carboxylic acid group
Gas pressure = atm pressure - height of mercury
Periods 8 and 9 - lanthanides and actinides
Orientation of orbital in space
COOH - ends in -oic acid

31. Electron affinity
Soluble except when containing Ag? - Hg2²? - or Pb²?
Periods 8 and 9 - lanthanides and actinides
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Covalent

32. Chlorine gas
4 bonding - 109.5° - sp³ hybridization
Deadly - yellow-green - weapon
PV = nRT - R = .0821
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

33. Sterling silver
Moles / L
Mixture of silver and copper
4 bonding - 109.5° - sp³ hybridization
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

34. Properties of molecular crystals and liquids

35. Fission
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Liquid at room temperature - used to make gasoline and solvents
Purple

36. Suspension
NH2 - ends in -amide
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Orientation of orbital in space

37. Radioactivity
Excess oxygen
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

38. SO4²? compounds are...
Soluble
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Bright yellow
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

39. Sigma bonds
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Decreased
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Orange

40. Petroleum
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Orange
CO - produced from incomplete combustion - very toxic
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

41. Sulfate ion
Bright yellow
No
SO4²?
Magnesium

42. Acids with more oxygen atoms are
4.5 to 8.3 - Red to blue
Stronger
Bright yellow
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

43. amphoteric
Same formula - different structure
Photography
Substance can act either as an acid or a base
Orange

44. Dipole-dipole forces (including hydrogen bonds)
Soluble
Spin is +1/2 or -1/2 in an orbital
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Yellow to orange

45. Fusion
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Decreased
Covalent

46. Color of Fe3+ solution
Yellow to orange
Make up jet fuels and kerosene
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Most stable

47. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Do not conduct electricity well
5 bonding - 90° and 120° - sp³d hybridization
SO4²?
Insoluble

48. Carbonate ion
Soluble except when containing Ag? - Hg2²? - or Pb²?
SO4²?
CO3²?
Covalent

49. Steel
R-O-R functional group - shorter chain ends in oxy - other is ane
COOH - ends in -oic acid
Mixture of iron and carbon
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

50. Litmus: pH range and colors
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
NO3?
4.5 to 8.3 - Red to blue
PV = nRT - R = .0821