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SAT Subject Test: Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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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. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Yes in thermo - no in electro
Orange
NH2 functional group - name ends in -amide

2. Add acid to water or water to acid
Soluble except when containing alkaline earth metals
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Acid to water
Mixture of tin - copper - bismuth - and antimony

3. Litmus: pH range and colors
Soluble
4.5 to 8.3 - Red to blue
Covalent
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

4. List equivalent pressure values for mmHg - torr - atm - and Pa
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
3 bonding - 120° - sp² hybridization
COOH functional group - name ends in oic acid
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

5. Hydrogen gas properties
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Involves water
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

6. bronze
SO4²?
Mixture of copper - zinc - and other metals
Properties of solutions that depend on the number of particles per solvent molecule
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

7. Sulfide color: CuS - HgS - and PbS
Purple/pink
Black
Strong acids - strong bases - soluble salts
Extremely slow reactivity

8. Ethanol
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
8.3 to 10.0 - colorless to pink
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Same formula - different structure

9. Complete combustion occurs when there is
Yellow to orange
Soluble
Excess oxygen
No

10. Color of excited Cu2+
V1/T1 = V2/T2
Stronger
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Blue-green

11. Pauli exclusion principle
OH functional group - name ends in -ol
yellow
No two electrons can have the same set of 4 quantum numbers
Insoluble

12. Gamma decay
Heat required to make a substance melt.
Emission of electromagnetic energy after beta - positron - or alpha decay
CO3²?
Green

13. Allotropic forms of carbon
Insoluble
Classified as strong bases but not very soluble.
Nonmetal oxides form acids - metal oxides form bases
Diamond - graphite - amorphous - fullerenes

14. Linear
Defines shape of orbital
2 bonding - 180° - sp hybridization
Endothermic
Liquid at room temperature - used to make gasoline and solvents

15. Color of Fe3+ solution
Mixture of copper and zinc
Yellow to orange
21% of atmosphere - colorless - odorless - supports combustion reactions
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

16. Isoelectronic
Orange
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
V1/T1 = V2/T2
Two atoms with the same number of electrons

17. 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
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
C2H3O2?

18. Bromthymol blue: pH range and colors
6.0 to 7.6 - yellow to blue
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Miscible with water - flammable - used as fuel - poisonous
Soluble except when containing Ag? - Hg2²? - or Pb²?

19. Amine group
SO4²?
NH2 - ends in -amide
Emission of electromagnetic energy after beta - positron - or alpha decay
Make up jet fuels and kerosene

20. How many joules are in a calorie?
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
4.184
Stronger
Black

21. Combustion reaction
Involves water
Increases left and down
Soluble except when containing alkaline earth metals
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

22. Properties of bases
Insoluble
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
A compound breaks into two parts
4.184

23. Colligative properties
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
COH functional group - name ends in -al
Stronger
Properties of solutions that depend on the number of particles per solvent molecule

24. Sulfate ion
Two compound react to form two new compounds
SO4²?
Gold
NO3?

25. Sulfide color: As2S3
NH4?
COOH functional group - name ends in oic acid
2 bonding - 1 nonbonding
Lemon yellow

26. Synthesis reaction
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Magnesium
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Two reactants combine to form a single product

27. Isotope
yellow
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
COH functional group - name ends in -al
Same element - different number of neutrons

28. Color of excited Ba2+
3 bonding - 120° - sp² hybridization
Light green
Substance can act either as an acid or a base
Covalent

29. Solute vs. Solvent
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Defines shape of orbital
The solute is dissolved in the solvent.
Mixture of iron and carbon

30. What qualifies as a strong base?
Most stable
4 bonding - 109.5° - sp³ hybridization
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Gas pressure = atm pressure - height of mercury

31. When a reaction is endothermic - the entropy is
Increased
Classified as strong bases but not very soluble.
A compound breaks into two parts
Orange

32. Cl - Br - and I compounds are...
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Mixture of silver and copper
Soluble except when containing Ag? - Hg2²? - or Pb²?
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

33. Color of MnO4? solution
2 bonding - 1 nonbonding
Purple
Moles of solute / kg solvent
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

34. What are the allotropic forms of sulfur?
Degrade the oxone layer
Low pressures - high temperatures
Soluble
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

35. Compounds with 5-10 carbons
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Liquid at room temperature - used to make gasoline and solvents
Covalent

36. Gibb's Free Energy equation
DG = DH - TDS
It is at equilibrium
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
CO3²?

37. Hydrolysis reaction
Lemon yellow
Yes
Involves water
Mixture of copper - zinc - and other metals

38. Petroleum
More active element replaces less active element in a compound.
OH functional group - name ends in -ol
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Magnesium

39. What metal will react in hot water?
Magnesium
Involves water
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Diamond - graphite - amorphous - fullerenes

40. Nitrate ion
3.1 - 4.4 - red to yellow
Solid at room temperature
NO3?
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

41. Suspension
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
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Purple/pink
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

42. Carboxylic acid group
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
COOH - ends in -oic acid
Gas pressure = atm pressure + height of mercury
Spin is +1/2 or -1/2 in an orbital

43. Electron affinity
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Excess oxygen
SO4²?
2 bonding - 1 nonbonding

44. amphoteric
Substance can act either as an acid or a base
Decreased
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

45. If G is zero - what is happening in the reaction?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
A compound breaks into two parts
It is at equilibrium
1st group - most reactive metal family - react violently with water - create basic solutions

46. Color of excited K+
PV = nRT - R = .0821
Purple/pink
Energy level - as it increases electrons are less bound to the nucleus
Bright yellow

47. Noble gas properties
Most stable
Same formula - different structure
Mixture of copper and zinc
Stronger

48. Ionic solids
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Two atoms with the same number of electrons
Limited oxygen
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

49. How can hydrogen be produced?
CO3²?
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Diamond - graphite - amorphous - fullerenes
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

50. Equation when using a barometer to calculate gas pressure.
Excess oxygen
Gas pressure = atm pressure - height of mercury
3 bonding - 120° - sp² hybridization
760 mmHg = 760 torr = 1 atm = 101 -325 Pa