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SAT Subject Test: Chemistry

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Answer 50 questions in 15 minutes.
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1. Color of Cu2+ solution
Defines shape of orbital
Blue
Light green
R-O-R functional group - shorter chain ends in oxy - other is ane

2. Nitrate ion
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.
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
NO3?

3. Boiling point elevation formula
Soluble
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
CO3²?
Orange

4. How many joules are in a calorie?
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Moles / L
4.184
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

5. Alchohols
OH functional group - name ends in -ol
Make up jet fuels and kerosene
Q = mcDT
3.1 - 4.4 - red to yellow

6. When the reaction is exothermic - the entropy is
Yes
Gold
Orange
Decreased

7. Coal
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
No two electrons can have the same set of 4 quantum numbers
Limited oxygen
2 bonding - 180° - sp hybridization

8. Positron emission
M1V1 = M2V2
CO - produced from incomplete combustion - very toxic
Yellow to orange
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

9. Colloid
Black
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
Moles / L
Increase right and up

10. Isotope
Extremely slow reactivity
NH4?
4.5 to 8.3 - Red to blue
Same element - different number of neutrons

11. Properties of molecular crystals and liquids

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12. Properties of acids
4.5 to 8.3 - Red to blue
3 bonding - 120° - sp² hybridization
Spin is +1/2 or -1/2 in an orbital
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

13. Electron affinity
CO3²?
Blue
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Gas pressure = atm pressure + height of mercury

14. Sterling silver
Mixture of silver and copper
Electrons are free to move through metal structure - high conductivity - ductile
A compound breaks into two parts
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

15. Metallic solids
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
Blue-green
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Solid at room temperature

16. Compounds with 12-18 carbons
Potassium - Calcium - Sodium
Orientation of orbital in space
Make up jet fuels and kerosene
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

17. Gamma decay
NO3?
Disordered systems with higher entropies are favored
Emission of electromagnetic energy after beta - positron - or alpha decay
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

18. Fission
PO4³?
21% of atmosphere - colorless - odorless - supports combustion reactions
Diamond - graphite - amorphous - fullerenes
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

19. Anhydride
Low pressures - high temperatures
Oxide that reacts with water to form either an acid or a base
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
No

20. Supersaturated solution
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
The solute is dissolved in the solvent.
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

21. Isoelectronic
COH functional group - name ends in -al
3 bonding - 120° - sp² hybridization
21% of atmosphere - colorless - odorless - supports combustion reactions
Two atoms with the same number of electrons

22. Alkali Metals
P1/V1 = P2/V2
Classified as strong bases but not very soluble.
Mixture of tin - copper - bismuth - and antimony
1st group - most reactive metal family - react violently with water - create basic solutions

23. Hydrogen gas properties
Blue
Miscible with water - flammable - used as fuel - poisonous
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Yes in thermo - no in electro

24. Gibb's Free Energy equation
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
DG = DH - TDS
Soluble except when containing alkaline earth metals

25. Carbonate ion
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
CO3²?
Mixture of tin - copper - bismuth - and antimony
Make up jet fuels and kerosene

26. bronze
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Heat required to make a substance melt.
Mixture of copper - zinc - and other metals

27. Chlorofluorocarbons
COOH functional group - name ends in oic acid
Degrade the oxone layer
Endothermic
Decreased

28. Amine
6 bonding - 90° - sp³d2² hybridization
Mixture of copper - zinc - and other metals
NH2 functional group - name ends in -amide
Extremely slow reactivity

29. Pi bonds
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
COH functional group - name ends in -al
Same formula - different structure
The solute is dissolved in the solvent.

30. Chlorate ion
Insoluble
4.5 to 8.3 - Red to blue
ClO3?
Deadly - yellow-green - weapon

31. Ammonium Ion
3 bonding - 1 nonbonding 107°
21% of atmosphere - colorless - odorless - supports combustion reactions
Increase right and up
NH4?

32. Exceptions to the octet rule
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Acid to water
21% of atmosphere - colorless - odorless - supports combustion reactions
P1/V1 = P2/V2

33. Carbon dioxide gas properties
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
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Etching glass and frosting lightblubs
NH4?

34. Graham's Law
Blue
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

35. Define heat of fusion.
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Heat required to make a substance melt.
Blue-green

36. amphoteric
Deadly - yellow-green - weapon
P1/V1 = P2/V2
Substance can act either as an acid or a base
M1V1 = M2V2

37. Examples of strong electrolytes
Gases at room temperature - used for fuel
Strong acids - strong bases - soluble salts
Soluble except when containing alkaline earth metals
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

38. Compounds with 1-4 carbons
Photography
NH2 - ends in -amide
C2H3O2?
Gases at room temperature - used for fuel

39. What 3 metals will react with cold water?
Potassium - Calcium - Sodium
Magnesium
7th group - form salts - always exist as diatomic molecules - used in modern lighting
3 bonding - 1 nonbonding 107°

40. Petroleum
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Soluble except when containing alkaline earth metals
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Yes

41. Covalent-network / atomic solids
SO4²?
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
The solute is dissolved in the solvent.
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

42. Linear
Liquid at room temperature - used to make gasoline and solvents
Purple
2 bonding - 180° - sp hybridization
Most stable

43. Sulfide color: Sb2S3
Orange
Electrons are free to move through metal structure - high conductivity - ductile
Liquid at room temperature - used to make gasoline and solvents
1st group - most reactive metal family - react violently with water - create basic solutions

44. Litmus: pH range and colors
Do not conduct electricity well
Red
ClO3?
4.5 to 8.3 - Red to blue

45. Spin quantum number (ms)
PO4³?
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Spin is +1/2 or -1/2 in an orbital
Nonmetal oxides form acids - metal oxides form bases

46. Halogens
White
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Decreased
7th group - form salts - always exist as diatomic molecules - used in modern lighting

47. Rare earth elements
The solute is dissolved in the solvent.
Periods 8 and 9 - lanthanides and actinides
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
Most stable

48. What are the factors that affect reaction rate?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Photography
ClO3?
Degrade the oxone layer

49. Colligative properties
7th group - form salts - always exist as diatomic molecules - used in modern lighting
4 bonding - 109.5° - sp³ hybridization
Properties of solutions that depend on the number of particles per solvent molecule
Green

50. Electronegativity
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Orange
Increase right and up
OH functional group - name ends in -ol

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SAT Subject Test: Chemistry

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