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SAT Subject Test: Chemistry

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Answer 50 questions in 30 minutes.
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Match each statement with the correct term.
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1. When are gases MOST ideal?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Strong acids - strong bases - soluble salts
Low pressures - high temperatures
Mixture of copper - zinc - and other metals

2. Carboxylic acid group
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
COOH - ends in -oic acid
Blue
Covalent

3. Fusion
Covalent
Strong acids - strong bases - soluble salts
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

4. Hydrogen gas properties
Gases at room temperature - used for fuel
2 bonding - 1 nonbonding
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Mixture of silver and copper

5. Sigma bonds
8.3 to 10.0 - colorless to pink
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
COH functional group - name ends in -al
Decreased

6. Synthesis reaction
DG = DH - TDS
NO3?
Two reactants combine to form a single product
Green

7. Gamma decay
Gas pressure = atm pressure + height of mercury
Classified as strong bases but not very soluble.
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Emission of electromagnetic energy after beta - positron - or alpha decay

8. Color of CrO4²? solution
Spin is +1/2 or -1/2 in an orbital
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Yellow
The solute is dissolved in the solvent.

9. Sulfide color: CdS
Extremely slow reactivity
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
Bright 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

10. Silver bromide and silver iodide are used for
Glass and plastic
Photography
Nonmetal oxides form acids - metal oxides form bases
R-O-R functional group - shorter chain ends in oxy - other is ane

11. Combustion reaction
Strong acids - strong bases - soluble salts
Yellow
Black
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

12. Molarity
It is at equilibrium
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Moles / L
4 bonding - 109.5° - sp³ hybridization

13. Atomic radius trend
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Increases left and down
Stronger

14. Freezing point depression formula
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Glass and plastic

15. How many joules are in a calorie?
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Increases left and down
Etching glass and frosting lightblubs
4.184

16. Isoelectronic
Gold
Soluble
Black
Two atoms with the same number of electrons

17. Properties of acids
Potassium - Calcium - Sodium
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Blue-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

18. Noble gas properties
Potassium - Calcium - Sodium
COH functional group - name ends in -al
Most stable
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

19. Color of MnO4? solution
DH = bonds broken - bonds formed
Purple
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Pressure of mixture of gases equals some of individual gas pressures.

20. Dilution equation
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Strong acids - strong bases - soluble salts
Gas pressure = atm pressure + height of mercury
M1V1 = M2V2

21. Oxygen gas properties
21% of atmosphere - colorless - odorless - supports combustion reactions
Orange
Soluble
Q = mcDT

22. Ionic solids
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
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Do not conduct electricity well

23. Aldehydes
OH functional group - name ends in -ol
Liquid at room temperature - used to make gasoline and solvents
COH functional group - name ends in -al
More active element replaces less active element in a compound.

24. Principal quantum number (n)
Yes in thermo - no in electro
Insoluble
M1V1 = M2V2
Energy level - as it increases electrons are less bound to the nucleus

25. Color of excited Na+
6 bonding - 90° - sp³d2² hybridization
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.
PO4³?
yellow

26. Color of Ni2+ solution
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
ClO3?
Green

27. Sulfide color: Sb2S3
OH - alcohols - name ends in ol
OH functional group - name ends in -ol
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.
Orange

28. Spin quantum number (ms)
Defines shape of orbital
Moles / L
Spin is +1/2 or -1/2 in an orbital
It is at equilibrium

29. Charles' Law
COOH functional group - name ends in oic acid
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
V1/T1 = V2/T2
Soluble except when containing Ag? - Hg2²? - or Pb²?

30. How can hydrogen be produced?
Substance can act either as an acid or a base
Light green
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
CO - produced from incomplete combustion - very toxic

31. Pauli exclusion principle
Periods 8 and 9 - lanthanides and actinides
Soluble
No two electrons can have the same set of 4 quantum numbers
Decreased

32. If G is positive - is the reaction spontaneous?
Lemon yellow
Orange
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
No

33. Compounds with 12-18 carbons
Make up jet fuels and kerosene
Same element - different number of neutrons
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Red

34. Add acid to water or water to acid
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Acid to water
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

35. Dipole-dipole forces (including hydrogen bonds)
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

36. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Soluble
R-O-R functional group - shorter chain ends in oxy - other is ane
Electrons are free to move through metal structure - high conductivity - ductile
Insoluble

37. Solute vs. Solvent
The solute is dissolved in the solvent.
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Degrade the oxone layer
NO3?

38. SO4²? compounds are...
The solute is dissolved in the solvent.
NH2 functional group - name ends in -amide
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
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

39. Compounds with 18 carbons
3.1 - 4.4 - red to yellow
Gases at room temperature - used for fuel
Solid at room temperature
Orientation of orbital in space

40. Isotope
21% of atmosphere - colorless - odorless - supports combustion reactions
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Same element - different number of neutrons
Mixture of tin - copper - bismuth - and antimony

41. What are the allotropic forms of sulfur?
Orange
Low pressures - high temperatures
ClO3?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

42. What qualifies as a strong base?
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Gas pressure = atm pressure - height of mercury

43. When the reaction is exothermic - the entropy is
Insoluble
Decreased
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Solid at room temperature

44. If G is zero - what is happening in the reaction?
Excess oxygen
Increased
No
It is at equilibrium

45. Ionization energy
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Properties of solutions that depend on the number of particles per solvent molecule
1st group - most reactive metal family - react violently with water - create basic solutions

46. Color of excited K+
Purple/pink
3.1 - 4.4 - red to yellow
CO3²?
Substance can act either as an acid or a base

47. Magnetic quantum number (ml)
Orientation of orbital in space
Pressure of mixture of gases equals some of individual gas pressures.
4 bonding - 109.5° - sp³ hybridization
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

48. Linear
2 bonding - 180° - sp hybridization
Stronger
6.0 to 7.6 - yellow to blue
Magnesium

49. Gibb's Free Energy equation
Two reactants combine to form a single product
DG = DH - TDS
Two compound react to form two new compounds
ClO3?

50. Halogen properties
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Disordered systems with higher entropies are favored

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Test your basic knowledge |

SAT Subject Test: Chemistry

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3d Computer Modeling

Actionscript

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Adobe Photoshop CS 5 Keyboard Shortcuts

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After Effects Keyboard Shortcuts

Agile Development

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Android Programming

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