Name_____________________________________________________________ Date________________ Period______ Bonding and Intermolecular Forces Guided Notes Use the textbook or Internet resource to find the following information. Polarity and Lewis Structures EQ: How does electronegativity of the elements in a bond relate to the polarity? EQ: How do you draw the Lewis structures of compounds? Lewis Structures and Bonding Valence electron Covalent bond Metallic bond Ionic bond Lewis structure Octet rule Lone pairs Electrostatic force Definitions: Indicate the number of valence electrons and charge for each group and draw the “staircase” that separates metals and nonmetals.
Bonding and Intermolecular Forces Guided NotesUse the textbook or Internet resource to find the following information.
Polarity and Lewis StructuresEQ: How does electronegativity of the elements in a bond relate to the polarity?EQ: How do you draw the Lewis structures of compounds?Lewis Structures and Bonding
Valence electron
Covalent bond
Metallic bond
Ionic bond
Lewis structure
Octet rule
Lone pairs
Electrostatic force
Explain using electron
Definitions:
Indicate the number of valence electrons and charge for each group and draw the “staircase” that separates metals and nonmetals.
configuration why an element’s charges can be predicted by its position on the periodic table.
Diatomic molecules
Why does hydrogen not follow the octet rule?
Write a higher order question for each image below.
Circle the correct option in each sentence: Core electrons (are/are not) included when drawing the Lewis structure. (Ionic/covalent) compounds will form by transferring valence electrons
resulting in the formation of ions. (Ionic/covalent) compounds will form by sharing valence electrons, and will
NOT result in the formation of charged ions.
Definition:
Elements that will form diatomic molecules:
Way to remember the elements that will form diatomic molecules:
_____________________bond:
___________________ bond:
**** VERY IMPORTANT: When drawing the Lewis structures you must draw ALL OF THE LONE PAIRS!! If you leave them off it WILL be marked completely wrong on the AP exam. No partial credit will be given at all!!
_____________________ bond:
Bond length
Bond energy
Polar covalent bond
Dipole moment
Polar molecule
Write at least 2 higher order questions relating to the graphic organizer:
How do you predict the type of
Define:
Complete the graphic organizer below:
The arrow indicates:
bond that forms between two elements using electronegativities of the elements involved?
Notation for polar molecules
How do you determine the direction the arrow points?
How do you determine which molecule is partially negative or partially negative?
Is it possible to have a molecule that is nonpolar, but contains polar covalent bonds? Justify your answer by drawing a picture and include an explanation.
The indicates:
**VERY IMPORTANT: when indicating a partial charge you MUST MUST MUST include the delta symbol. If you just write + or – you are saying that they are ions and this is not the case!! It will be marked completely wrong if you do this!!!!!!
Indicate if the molecules are polar or nonpolar and show the partial negative and partial positive charges on each molecule if applicable:
Summary:
Covalent bonding, VSEPR Theory, and HybridizationEQ: How do you determine the molecular shape, bond angle and hybridization of a molecule using VSEPR theory?
Valence shell electron-pair Define:
repulsion (VSEPR) model
Bond angle
Sigma bond
Pi bond
Hybridization
Write a higher order question for each table below:
Fill in the following tables:
Covalent network solids
Why does carbon tend to form covalent network solids?
Allotrope
Why is the boiling point of graphite high?
What type of intermolecular force is responsible for the attraction between the layers?
Explain why graphite is soft by describing the intermolecular forces.
Diamond is another allotrope of carbon. Suggest why diamond is harder than graphite.
Definition:
Covalent network solids only form from (metals/nonmetals) Melting points are (high/low) because
3D structures tend to be rigid due to fixed bond angles.
Define:
Answer the questions using the image below.
Summary:
Intermolecular ForcesEQ 1: What intermolecular forces are present in various molecules?EQ 2: How do the presence of different intermolecular forces affect the boiling point, vapor pressure, capillary action, solubility, or surface tension?
Intermolecular force
How do intermolecular forces differ from chemical bonds?
Definition:
Dipole-dipole attraction
Dipole-induced dipole attraction
Hydrogen bonding
Definition:
Occurs between (polar/nonpolar) molecules. Relative strength:
Definition:
An induced dipole is
Occurs between
Relative strength:
Definition:
Occurs between (polar/nonpolar) molecules. A strongly electronegative element such as ________________________ and
___________________ must be present in order for hydrogen bonding to occur.
How would methane’s (CH4) boiling point differ from butane (C4H10)? Justify your answer. Be sure to identify which IMF are present in the molecules and indicate which molecule will have stronger IMF.
Vapor pressure
Definition:
Occurs between (polar/nonpolar) molecules. Results from an (instantaneous/permanent) dipole. Electron clouds shift to one side producing a partial charge. Relative strength:
Larger molecules have (stronger/weaker) London dispersion forces because
Strong IMF would cause a (higher/lower) boiling point because
Capillary action
Surface Tension
Solubility
Definition:
Stronger IMF would cause a (higher/lower) vapor pressure because
Definition:
Stronger IMF would cause a (higher/lower) vapor pressure because
Definition:
Stronger IMF would cause (higher/lower surface tension because
Definition:
Strong IMF would cause higher/lower solubility because
Explain the rule “like dissolves like”:
Summary:
Ionic Bonding and Crystal LatticesEQ: How are ionic compounds arranged into a crystal lattice?EQ: How does the relative lattice energy predict the solubility of a salt?
Coulomb’s law
Ionic solid
Molecular solid
Crystal lattice
Lattice energy
Can an ionic compound be considered a polar molecule? Use definitions to justify your answer.
How does Coulomb’s law relate to the strength of the lattice energy in an ionic solid?
Use the image to the right to answer the following questions:
Which compound would have greater lattice energy? Justify your answer.
Why are the sodium and magnesium ions drawn smaller than the oxygen and fluorine atoms?
Solute
Fill in the blanks: In an ionic bond, _________________________ are transferred from a metal
to a nonmetal. The transfer results in the formation of ____________________. The electrostatic (Coulombic) attraction between ions results in the formation
of a crystal lattice.
Define:
Solvent
Why is the sodium ion smaller than the chloride ion? Justify your answer using a description of the Coulombic attractions within the molecule.
Would the water molecules have a greater attraction to the sodium ion or the chloride ion? Justify your answer by describing Coulombic attractions.
If magnesium ions were added to the solution drawn above, would the water molecules have a stronger attraction to the magnesium or sodium ions? Justify your answer using an explanation of Coulombic attractions between particles.
Greater lattice energy results in (higher/lower) solubility. When an ionic compound dissolves, it breaks up into its ions. Ion charges can be predicted from the element’s position on the
___________________________________. When NaCl dissolves in water, the ions that result are:
When MgF2dissolves in water, the ions that result are:
Water is a (polar/nonpolar) molecule. Due to Coulomb’s law, the (partially positive/partially negative) side of the
water molecule would be attracted to positive ions.
Complete the image below by drawing in at least 5 water molecules around the ions to correctly show the attractions in sodium chloride solution. BE SURE TO INCLUDE THE PARTIAL POSITIVE AND PARTIAL NEGATIVE CHARGES WHERE APPLICABLE.
Summary:
Metallic Bonding and AlloysEQ: How do the properties of various alloys relate to the molecular structure and the electron sea model of metal solids?
Conductivity
Malleability
Ductility
Interstitial alloy
Substitutional alloy
Oxide layer
Explain why metals are conductive, malleable and ductile using the electron sea model.
Explain why alloys tend to be less malleable and ductile than pure metals.
Define:
Draw a picture of the electron sea model below. Indicate the positive cores and the mobile valence electrons.
Summary:
Separation TechniquesEQ: How can solutes be separated based on their intermolecular forces?Filtration
What type of mixtures will be successfully separated using filtration?
Chromatography
Definition:
Filtration will separate mixtures based on particle size. Large particles will be trapped in the filter paper while small particles will be able to pass through.
FILTRATION WILL NOT SEPARATE DISSOLVED SOLIDS FROM A MIXTURE! (Ions = very small)
Definition:
Setup for paper chromatography:o Origin line is drawn on chromatography paper using a
____________________ to mark where the ink dot is placed.o The bottom of the chromatography paper is placed in the solvent.o The ink should not touch the solvent initially.o The dyes are allowed to separate.
Separates based on the differential strength of IMF. More separation = (weaker/stronger) IMF between the solute and solvent. Polar substances will have a (weaker/stronger) attraction to water
Using chromatography, how would you tell if a dye is a pure substance?
Rf value
If you determine the Rf value of an illegal dye, how can you use paper chromatography to show that it is being used in a dye mixture used to color candy?
Distillation
When solvent is polar:
Definition:
Separates chemical species by taking advantage of the differential strength of IMF between and among components and the effects these interactions have on vapor pressures of the components.
What is the purpose of the cold water moving through the condensing tube?
What interactions exist between the positive and negative ions shown in the image above?
What interactions exist between the water molecules shown in the image above?
Is the interaction between ions or the interaction between water molecules stronger? Justify your answer.
