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PRACTICE TEST – Chemical Bonding (3rd Test) Name: __________________________ 75 points + 3 EC = 104% possible 1-2) Complete the following problems for Magnesium and Phosphorus 5 points Magnesium (Neutral ) Ve- =___ __ e- = __ P+ =__ Ve- =___ __ e- = __ P+ =__ 12 3 Phosphorus (Neutral) New Ion Symbol Lewis Structure e- = __ P+ =__ 12 Magnesium What must be done to make this atom stable? 12 Ve- =___ __ New Ion Symbol Lewis Structure 3 Phosphorus e- = __ Ve- =___ __ P+ =__ What must be done to make this atom stable? 12 3 3 Complete the table for both Monatomic & Polyatomic Ions below: 6 points = ½ point each Name Ion Charge Name Ion Charge + 3) sulfite 7) NH4 4) sulfide 8) O2- 5) hydroxide 9) CO3 2- 6) phosphide 10) Cu2+ Identify each as either ionic or covalent compounds and provide either the name or formula You may find these prefixes helpful for the questions below mono- di- tri- tetra- penta hexa- hepta octa- nona- deca- 1 2 3 4 5 6 7 8 9 10 Ionic or Covalent 11) dinitrogen trioxide 12) MgF2 13) phosphorus trifluoride 14) sulfur dioxide 15) N2O5 16) calcium nitrate 17) CO 18) lead (IV) oxide 19) FeSO4 20) H2O Name or Formula 8 pts = ½ ea Identify each characteristic as being part of an IONIC Bond or a COVALENT Bond: 6 points 21) _____________- Typically solids at room temperature 22) _____________- Usually have high melting and boiling points 23) _____________ -Bonding occurs when there is a transfer valence electrons 24) _____________- Bonding occurs between nonmetals and metals 25) _____________- Compounds have relatively weak force of attraction between molecules 26) _____________- Bonding occurs between nonmetals and nonmetals 27) _____________- When dissolved in water, it will conduct electricity 28) _____________- Bonding occurs when there is a sharing of valence electrons Match each item with the correct statement below. NOTE: Each item may be used once, more than once, or not at all. A. B. C. D. E. F. cation anion polyatomic ion ionic compound molecular compound net charge of Zero G. electron configuration H. electrostatic force I. octet rule J. valence electrons K. electron dot structure (Lewis Structure) M. ionic bond N. metallic bond O. single covalent bond Q. double covalent bond R. crystal lattice ____ 29. the force of attraction between a positive and negative charge ____ 30. the element oxygen will gain two electrons to form a(n) ___________ ____ 31. the arrangement of electrons around the nucleus of an atom in its ground state ____ 32. atom or group of atoms having a positive charge ____ 33. a repeating pattern of cations and anions bonded together ____ 34. tightly-bound group of atoms that behaves as a unit and carries a net charge ____ 35. type of compound that forms a crystal lattice ____ 36. a covalent bond in which only one pair of electrons is shared ____ 37. type of compound composed only of non-metals that are covalently bonded together ____ 38. atoms react so as to acquire the stable electron structure of a noble gas with a full valence shell ____ 39. this type of bond is found in a molecule of water (H2O) ____ 40. a depiction (drawing) of valence electrons around the symbol of an element ____ 41. the electrons in the highest occupied energy level of an atom (outer most energy level) ____ 42. atom or group of atoms having a negative charge ____ 43. the electrostatic attraction between a sea of freely flowing valence electrons and metal cations ____ 44. when the total positive charge of the cation is equal to the total negative charge of the anion ____ 45. this type of bond is found in table salt (NaCl) ____ 46. a covalent bond in which two pairs of electrons are shared ____ 47. phosphate PO43- is an example of a(n) _________ ____ 48. the electrostatic force of attraction binding oppositely charged ions together ____ 49) What is the ionic charge on the Vanadium ion in the ionic compound Vanadium Sulfide, VS ? ____ 50) How many total covalent bonds will a nitrogen atom form in order to become stable? ____ 51) How many electrons does carbon need to share in order to obtain a noble-gas electron configuration? ____ 52) What is the charge on the cation in FeCO3? ____ 53) What is the net charge of the ionic compound sodium oxide? ____ 54) Which of the following elements does NOT form an ion with a charge of 2+ ? a. magnesium b. calcium c. oxygen d. copper (II) ____ 55) Which of the following particles are free to drift in metals? a. protons b. electrons c. neutrons d. cations ____ 56) Which of the following pairs of elements is most likely to form an ionic compound? a. chlorine and oxygen c. aluminum and chlorine b. nitrogen and sulfur d. sodium and lithium ____ 57) Which of the following is true about the melting temperature of dihydrogen monoxide? a. The melting temperature is relatively high. c. The melting temperature is relatively low. b. The melting temperature is variable and unpredictable. d. Dihydrogen monoxide does not melt. ____ 58) What characteristic of metals makes them good electrical conductors? a. They have mobile valence electrons. c. They have mobile cations. b. They have mobile protons. d. Their crystal structures can be rearranged easily. ____ 59) Which of these elements does not exist as a diatomic molecule? a. H b. F c. Ar d. O ____ 60) Which of the following correctly provides the correct name and formula for each acid? a. Carbonic Acid – HCO3 c. Hydrochloric acid – H2Cl b. Acetic Acid – HC2H3O2 d. Hydrophosphoric acid – H3PO4 ____ 61) How do atoms achieve noble-gas electron configurations (stability) in double covalent bonds? a. Two atoms share one electron. c. Two atoms share two pairs of electrons. b. Two atoms share two electrons. d. One atom completely loses two electrons to the other atom. ____ 62) Sulfuric Acid is written as: a. H2SO4 b. H2SO3 c. HS2 d. none of the above ____ 63) What is the basis of a metallic bond? a. the attraction of metal cations to mobile electrons b. the attraction between neutral metal atoms c. the neutralization of protons by electrons d. the attraction of oppositely charged ions ____ 64) Which noble gas has the same electron configuration as the oxygen atom in a water molecule? a. helium b. neon c. argon d. xenon ____ 65) Why do atoms share electrons in covalent bonds? a. to become ions and attract each other c. by gaining or losing electrons to become stable b. to attain a stable noble-gas electron configuration d. to increase their atomic numbers ____ 66) Which of the following is not one of the seven diatomic elements? a. O b. Cl c.He2 d. N ____ 67) What type of ions have names ending in -ide? a. only monatomic cations b. only monatomic anions c. only metal ions ____ 68) When Group 6A elements form ions, they ____. a. lose two protons b. gain two protons c. lose two electrons d. gain two electrons ____ 69) When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a ____. a. prefix c. roman numeral following the name b. suffix d. superscript after the name ____ 70) How are chemical formulas of ionic compounds generally written? a. subscripts first, then ions c. Roman numeral first, then anion, then cation b. cation on left, anion on right d. anion on left, cation on right ____ 71) Which of the following is NOT an anion? a. hydroxide b. sulfate c. ClO1- d. iron(III) ion ____ 72) Which of the following is true about the composition of ionic compounds? a. They are composed of cations and anions. c. They are composed of cations only. b. They are composed of anions only. d. They are formed from two or more nonmetallic elements. ____ 73) Which element, when combined with bromine, would most likely form an ionic compound? a. lithium b. carbon c. phosphorus d. chlorine ____ 74) What type of compound is CaO? a. binary ionic b. polyatomic covalent c. polyatomic ionic d. binary molecular ____ 75) Which type of bond has the strongest electrostatic force of attraction between the atoms? a) Metallic b. ionic c. covalent d. all three have the same amount of electrostatic force ____ 76) Which of the following compounds would require the most amount of energy to break the bonds a. single bond b. double bond c. triple bond d. they would all require the same amount of energy ____ 77) Which of the following is true about the melting temperature of potassium chloride? a. The melting temperature is relatively high. c. The melting temperature is relatively low. b. The melting temperature is variable and unpredictable. d. Potassium chloride does not melt. ____ 78) Which of the following formulas represents a molecular compound? a. Ar b. CO32c. CuOH d. NO ____ 79) What does an -ite or -ate ending in a polyatomic ion mean? a. Bromine is in the formula. c. Nitrogen is in the formula. b. Sulfur is in the formula. d. Oxygen is in the formula. ____ 80) A repeating patterns of positive and negative ions held together by electrostatic attraction is a(n) a. polyatomic ion b. crystal lattice c. diatomic molecule d. single covalent bond ____ 81) Which of the following formulas represents an ionic compound? a. CS b. BaI c. N O d. PCl ____ 82) Which of the following compounds contains the lead(II) ion? a. PbO b. PbCl4 c. Pb2O d. Pb2S ____ 83) The octet rule states that, in chemical compounds, atoms tend to have ____. a. the electron configuration of a noble gas c. more protons than electrons b. eight electrons in their first (principal) energy level d. more electrons than protons ____ 84) What is the charge of the ion formed when potassium achieves noble-gas electron configuration? a. K4+ b. K+ c. K1d. K2____ 85) Which of the following elements does NOT form an ion with a charge of 1+ ? a. fluorine b. hydrogen c. potassium d. sodium ____ 86) How can you determine if a compound is an acid? a. there is an oxygen atom in the formula b. the first element is a hydrogen atom b. the net charge will be zero d. it will have both a metal and a non-metal ____ 87) Which of the following occurs in an ionic bond? a. Oppositely charged ions attract. c. Two atoms share more than two electrons. b. Two atoms share two electrons. d. Like-charged ions attract. ____ 88) What is the net charge of the ionic compound calcium fluoride? a. 2– b. 1– c. 0 d. 1 ____ 89) What is the name of the ionic compound formed from lithium and bromine? a. lithium bromine b. lithium bromide c. lithium bromium d. lithium bromate ____ 90) Which of the following compounds has the formula KNO ? a. potassium nitrate b. potassium nitride c. potassium nitrite d. potassium nitrogen oxide ____ 91) Which of the following pairs of elements is most likely to form an ionic compound? a. magnesium and fluorine c. oxygen and chlorine b. nitrogen and sulfur d. sodium and aluminum ____ 92) In which of the following is the name and formula given correctly? a. sodium oxide, NaO c. cobalt (II) chloride, CoCl b. barium nitride, BaN d. tin(II) fluoride, SnF 2 93) What does an atom react? 95) What are the seven diatomic elements? 96) Explain why Mono-atomic atoms do not bond. Provide an example of a mono-atomic atom. 3 points 97) Compare and Contrast Ionic and covalent bonds. 3 points a) how are they similar? b) how are they different? 98) Complete the Lewis Structures for each Compound 4 points Cl2 ____________ N2 ____________ C2H4 ___________ 99) What is a precipitate? 100) During the “Hydrogen Gas Lab” what was some observable evidence that a chemical reaction was occurring? pearsongreatpath.wikispaces.com