PRACTICETEST – Inter Molecular ForcesName: ______
Identify each as either ionic or covalent compounds and provide either the name or formula6 points
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
Name or Formula / Ionic or Covalent / Cation & Anion / Name or Formula
ex) nitrogen trihydride / Covalent / N/A - Covalent / NH3 (also known as ammonia)
ex) (NH4)2CO3 / Ionic / 2 NH41+ 1 CO32- / Ammonium Carbonate
1) calcium hydroxide
2) CO
3) carbon tetrahydride
4) Iron (III) Nitrate
5) MgSO4
6) Co(OH)2
Identify each of the Bond Types as either: Nonpolar Covalent, Polar Covalent, or Ionic
(Do not forget to include the identification of cations and anions or partial positive and partial negative where appropriate.)
6 points
7) HO 8) HI
(Identification) (Bond Type) (Identification) (Bond Type)
9) MgO / 11) HF10) NH / 12) O-O
13) Complete the Lewis Structures for each compound below, but sure to show the electrons for each atom and how the valence electrons overlap to indicate each covalent bond. 6 points
Polar or Nonpolar Polar or Nonpolar Polar or Nonpolar
14) For each item above (#13), indicate (circle) if the molecule is a polar molecule or non-polar molecule
15) Circlethe molecular structure of CH3OH
18) Explain “how” atoms become partially positive and partially negative in a polar bond. 2 points
Match each item (a-o) with the correct statement below. 10 points
(NOTE: each item (a-o) may be used once, more than once, or not at all).
a. cation f. ionic bondl. Van der Waals force
b. aniong. polar covalent bondm. London dispersion force (LDF)
c. electrostatic force h. nonpolar covalent bondn. dipole-dipole interaction (DDI)
d. electronegativityj. intramolecular forceo. hydrogen bond (HF)
e. dipole (polar molecule)k. intermolecular force
____ 19. the force of attraction between a positive and negative charge
____20. the electrostatic force between atoms – (covalent bond between atoms)
____21. the electrostatic force between molecules – cause molecules to stick to each other
____22. atom or group of atoms having a positive charge
____23. intermolecular force between molecules that have permanent dipolesthat are attracted to each other
____24. the relative ability of a bonded atom of an element to attract the electrons from the another element participating in the bond.
____25. a molecule that has two electrically charged regions (a slightly positive region and a slightly negative region)
____26. these forces are present in all molecules, whether they are polar or nonpolar.
____27. the electrostatic force of attraction binding oppositely charged ions together
____28. a covalent bond between two atoms of significantly different electronegativities – (bonding occurs when the electrons are shared unequally.)
____29. atom or group of atoms having a negative charge
____30. a covalent bond between atoms where the bonding electrons are shared equally.
____31. intermolecular force between an instantaneous dipole and an induced dipole. (Caused by the motion of the electrons)
____32. this type of intermolecular force is found between molecule of water (H2O)
____33. the dipole-dipole interactions experienced between molecules when H is bonded to N, O, or F
____34. in a polar covalent bond, the atom with the higher ______will become partially negative
____35. the weak attractive forces that hold molecules together (includes London dispersion, dipole-dipole interactions and hydrogen bonds)
____36. the force of attraction within ionic, metallic, and covalent bonds, hydrogen bonds, dipole-dipole interactions, London dispersion forces, and even between protons & electrons is due to ______.
Identify each of the following as either intermolecular or intramolecular 4 points
37) ______Polar Covalent Bond40) ______Ionic Bond
38) ______Hydrogen Bond41) ______Dipole-Dipole Interact
39) ______London Dispersion42) ______Van der Waals
42) For each box below, identify (label) the intermolecular and intramolecular attractions 4 points
____ 43) Which of the following covalent bonds is the most polar?
a. H—Fb. H—C c. H—Hd. H—N
____ 44) Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen?
a. Cb. Nc. Od. S
____ 45) Which of the forces of molecular attraction is the weakest?
a. dipole-dipole interaction b. London dispersion c. hydrogen bond d. single covalent bond
____ 46) Why do atoms share electrons in covalent bonds?
a. to become ions and attract each otherc. to become more polar
b. to gain a higher electronegativityd. to attain a full valence energy level
____ 47) A bond formed between a silicon atom and an oxygen atom is likely to be ____.
a. ionicb. coordinate covalent c. polar covalentd. nonpolar covalent
____ 48) What is thought to cause the London dispersion forces?
a. attraction between ionsc. sharing of electron pairs
b. motion of electronsd. differences in electronegativity
____ 50) Why is hydrogen bonding only possible with hydrogen?
a. Hydrogen’s nucleus is electron deficient when it bonds with an electronegative atom.
b. Hydrogen is the only atom that is the same size as an oxygen atom.
c. Hydrogen is the most electronegative element.
d. Hydrogen tends to form covalent bonds.
Identify the primary type of Van der Waals Forces that exist between each type of molecule:
LDF = London Dispersion Forces, DDI= Dipole-Dipole Interaction, HB = Hydrogen Bonds 10 points
63) List and explain the two factors that affect the force of attraction in London dispersion forces?2 points
64) Explain how London dispersion forces cause molecules to be attracted to one another. 2 points
65) Rank the following FOUR molecules from lowest to highest boiling points: EXPLAIN 2 points
CH4 CBr4CCl4CF4
66) Rank the following THREEmolecules from lowest to highest boiling points: EXPLAIN 2 points
67) Rank the following THREEmolecules from lowest to highest boiling points: EXPLAIN 2 points
68) What is the difference between a hydrogen bond and a polar covalent bond involving hydrogen?
69) Complete the table below using the following terms: (Solid, Liquid, Gas, Exothermic, Endothermic)
Phase Change / From / To / Endothermic or ExothermicDeposition / Gas / Solid / Exothermic (Gas is losing energy)
Sublimation
Freezing
Melting
Condensation
Vaporization
4points
70) TRUE or FALSE:Gases have an indefinite shape and a definite volume.
71) TRUE or FALSE:The motion/speed of the particles increasesas the temperature of particles decreases.
72) TRUE or FALSE:Because the shape of a solid never changes, the particles of the solid do not move.
73) TRUE or FALSE:Particles can stick together because of the intermolecular forces between the particles.
74) TRUE or FALSE:It is possible to heat pure water to a temperature of 127 °C.
75) TRUE or FALSE:Energy is either absorbed (Exothermic) or released (Endothermic) during a phase change.
76) TRUE or FALSE:The temperature of a substance changes during a phase change (melting/boiling).
77) TRUE or FALSE:The freezing point of and the melting point of a substance is the same temperature.
78) You put your recently washed, wet clothes into the dryer and start the machine. Forty-five minutes later,
your clothes are dry. What happened to the water?
79) A piece chocolate is sitting on the dashboard of your car on a hot sunny day.
80) After taking a hot shower, the mirror in the bathroom is all steamy (covered in water droplets). Explain how the mirror became wet. (Be sure to use the proper scientific terms in your response)
81) EXPLAIN what is happening at theatomic levelwhen a substance undergoes a phase change? Details required.