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SAT Subject Test: Chemistry

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Answer 50 questions in 15 minutes.
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1. Ester
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Yes
Etching glass and frosting lightblubs
Moles of solute / kg solvent

2. Exceptions to the octet rule
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Properties of solutions that depend on the number of particles per solvent molecule
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

3. Sulfide color: As2S3
Lemon yellow
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Moles / L
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

4. Complete combustion occurs when there is
R-O-R functional group - shorter chain ends in oxy - other is ane
Stronger
Excess oxygen
Orange

5. Color of Cu2+ solution
Blue
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Insoluble
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

6. Colloid
Degrade the oxone layer
2 bonding - 180° - sp hybridization
6.0 to 7.6 - yellow to blue
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

7. Gibb's Free Energy equation
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
DG = DH - TDS
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Oxide that reacts with water to form either an acid or a base

8. Phosphate ion
More active element replaces less active element in a compound.
Red
Etching glass and frosting lightblubs
PO4³?

9. Nonmetals
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
C2H3O2?
Do not conduct electricity well

10. What kind of bonds generally hold gases together?
Do not conduct electricity well
Covalent
Diamond - graphite - amorphous - fullerenes
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

11. Hydrofluoric acid is used for
Increased
Etching glass and frosting lightblubs
Yes
Properties of solutions that depend on the number of particles per solvent molecule

12. Radioactivity
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
P1/V1 = P2/V2
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
CO - produced from incomplete combustion - very toxic

13. Color of excited K+
Gas pressure = atm pressure - height of mercury
Purple/pink
6.0 to 7.6 - yellow to blue
Limited oxygen

14. What 3 metals will react with cold water?
4.5 to 8.3 - Red to blue
6.0 to 7.6 - yellow to blue
Potassium - Calcium - Sodium
The solute is dissolved in the solvent.

15. Ammonium Ion
NH4?
Defines shape of orbital
Light green
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

16. Compounds with 5-10 carbons
Gold
Liquid at room temperature - used to make gasoline and solvents
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Photography

17. Charles' Law
Two compound react to form two new compounds
Yes in thermo - no in electro
3 bonding - 120° - sp² hybridization
V1/T1 = V2/T2

18. Noble gas properties
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
OH - alcohols - name ends in ol
Most stable
Degrade the oxone layer

19. If G is negative - is the reaction spontaneous?
DH = bonds broken - bonds formed
Yes
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Orientation of orbital in space

20. Color of MnO4? solution
R-O-R functional group - shorter chain ends in oxy - other is ane
Purple
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Disordered systems with higher entropies are favored

21. Chlorine gas
P1/V1 = P2/V2
Low pressures - high temperatures
Deadly - yellow-green - weapon
Potassium - Calcium - Sodium

22. Spin quantum number (ms)
Spin is +1/2 or -1/2 in an orbital
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
NO3?
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

23. What is the second law of thermodynamics?
CO3²?
Disordered systems with higher entropies are favored
Orange
4 bonding - 109.5° - sp³ hybridization

24. Chlorate ion
ClO3?
NH4?
Mixture of tin - copper - bismuth - and antimony
Energy level - as it increases electrons are less bound to the nucleus

25. Compounds with 12-18 carbons
Purple/pink
Covalent
Make up jet fuels and kerosene
4.5 to 8.3 - Red to blue

26. Fission
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
yellow
ClO3?
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

27. When are gases MOST ideal?
Low pressures - high temperatures
Insoluble
Pressure of mixture of gases equals some of individual gas pressures.
7th group - form salts - always exist as diatomic molecules - used in modern lighting

28. Freezing point depression formula
Substance can act either as an acid or a base
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Same formula - different structure
Strong acids - strong bases - soluble salts

29. Covalent bond
Defines shape of orbital
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Mixture of iron and carbon
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.

30. Alkaline earth metals
2nd group - fairly reactive - pastes are used in batteries
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
M1V1 = M2V2
It is at equilibrium

31. Alkali Metals
7th group - form salts - always exist as diatomic molecules - used in modern lighting
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
1st group - most reactive metal family - react violently with water - create basic solutions
It is at equilibrium

32. Electronegativity
A compound breaks into two parts
Limited oxygen
Increase right and up
Mixture of tin - copper - bismuth - and antimony

33. Rare earth elements
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Periods 8 and 9 - lanthanides and actinides
Purple/pink
Classified as strong bases but not very soluble.

34. F compounds are...
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Soluble except when containing alkaline earth metals
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Orange

35. Sigma bonds
NH4?
21% of atmosphere - colorless - odorless - supports combustion reactions
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Defines shape of orbital

36. Ethers
R-O-R functional group - shorter chain ends in oxy - other is ane
OH functional group - name ends in -ol
Same molecule - different electron pair positions
CO - produced from incomplete combustion - very toxic

37. Litmus: pH range and colors
4.5 to 8.3 - Red to blue
NO3?
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Electrons are free to move through metal structure - high conductivity - ductile

38. Azimuthal quantum number (l)
2 bonding - 1 nonbonding
Defines shape of orbital
8.3 to 10.0 - colorless to pink
Potassium - Calcium - Sodium

39. What is the equation used for heat transfer problems?
Gas pressure = atm pressure + height of mercury
Q = mcDT
Decreased
3 bonding - 120° - sp² hybridization

40. Trigonal planar
Photography
3 bonding - 120° - sp² hybridization
A compound breaks into two parts
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

41. Positron emission
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
21% of atmosphere - colorless - odorless - supports combustion reactions
Mixture of tin - copper - bismuth - and antimony
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

42. Resonance structures
Soluble except when containing Ag? - Hg2²? - or Pb²?
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
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
Same molecule - different electron pair positions

43. Octahedral
Spin is +1/2 or -1/2 in an orbital
6 bonding - 90° - sp³d2² hybridization
Two atoms with the same number of electrons
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

44. List equivalent pressure values for mmHg - torr - atm - and Pa
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Decreased
Two compound react to form two new compounds
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

45. Define heat of fusion.
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Heat required to make a substance melt.
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
NH4?

46. Dalton's Law
Moles / L
Pressure of mixture of gases equals some of individual gas pressures.
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

47. Gamma decay
Solid at room temperature
Mixture of copper - zinc - and other metals
Mixture of iron and carbon
Emission of electromagnetic energy after beta - positron - or alpha decay

48. Trigonal bipyramidal
Lemon yellow
5 bonding - 90° and 120° - sp³d hybridization
Emission of electromagnetic energy after beta - positron - or alpha decay
Mixture of silver and copper

49. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Yes in thermo - no in electro
R-O-R functional group - shorter chain ends in oxy - other is ane
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Miscible with water - flammable - used as fuel - poisonous

50. Oxides are insoluble and when reacted with water..
Etching glass and frosting lightblubs
CO - produced from incomplete combustion - very toxic
Nonmetal oxides form acids - metal oxides form bases
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

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SAT Subject Test: Chemistry

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