Ch. 11 Flashcards (Intermolecular forces, Physical Properties, Solids) Flashcards Quizlet PDF

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Summary

Write succinctly, with a simple sentence structure. Minimise the use of adjectives.
results, eb x vg is autosomal; therefore, state the results indicate this. Therefore, you do not need to separate the results of each reciprocal cross – just state the totals.
Discussion – do not repeat ...

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Ch. 11 FLASHCARDS (Intermolecular forces, Physical Properties, Solids) Terms in this set (25) The intermolecular

London Dispersion Force (Induced dipole)

force(s) present in CH4, SiH4, GeH4, SnH4 is/are __________.

ALL atoms and

Induced Dipole Forces (London Dispersion Forces)

molecules have _____________ because they have electrons. There is random movement of electrons in a cloud which produce a temporary dipole or dispersal of electrons in a neighboring molecule

The reason that CH4,

CH4 has smaller electron clouds, so is less

has much lower boiling

polarizable (its induced dipole forces are weaker)

point than SnH4 is because

This IMF occurs in polar molecules. Positive end of one molecule is attracted to the negative end of an adjacent molecule.

Dipole/Dipole Interaction

Elemental iodine (I2) is a

Relatively strong London Dispersion Forces (due to

solid at room

large atoms)

temperature. What is the major attractive force that exists among different I2 molecules in the solid?

Which one of the

C. H2S (not polar enough to form H bonds)

following substances will NOT have hydrogen bonding as one of its intermolecular forces? A) HF B) NH3 C. H2S D. H2O

Polar ICl has a boiling

In this case, the London Dispersion Forces of the

point of 92 C. Nonpolar

octane are actually stronger (due to the large size

octane C8H18 has a

of the molecule) than the dipole/dipole interactions

boiling point of 125 C.

of the ICl.

How would you account for this observation?

What IMF is (are)

London Dispersion Forces, dipole/dipole

present in methanol

interactions and Hydrogen Bonding.

CH3OH?

(Hydrogen Bonding is the strongest however)

The predominant

(B) hydrogen bonding

intermolecular force in (CH3)2NH is __________. A) ion-dipole forces B) hydrogen bonding C) ionic bonding D) dipole-dipole forces E) London dispersion forces

A liquid begins to boil

vapor pressure..........atmospheric pressure

when its __________________equalizes or overcomes the surrounding ___________________.

Strong intermolecular forces in a substance are manifested by __________. A) high critical temperatures (the highest temp. that a substance can be found as a liquid) B) high boiling point C) low vapor pressure D) high heats of fusion and vaporization E) all of the above

E - all of these

In general, the vapor

decrease............higher..........lower

pressure of a liquid increases as the strength of the intermolecular forces ________________. So you would expect butane C4H10 to have a _____________vapor pressure than water, and a _______________boiling point than water.

The enthalpy change for

[10.0 g x .00418 kJ/g C x 75 C] + [ 40.67 kJ x .55 mol] +

converting 10.0 g of

[10.0 g x 0.00184 kJ/g C x 35.0 C] = 26.2 kJ

water at 25.0 C to steam at 135.0 C is ________ kJ. The specific heats of ice, water, and steam are 2.09 J/g-C, 4.18 J/gC, and 1.84 J/g-C, respectively. For H2O, ∆Hfus = 6.01 kJ/mol, and ∆Hvap = 40.67 kJ/mol. (Hint, sketch a segmented heating curve to guide your calculations and watch units!!!)

The principal source of

Br2 has a lower boiling point because the

the difference in the

Dispersion Forces among the Br2 molecules are

normal boiling points of

weaker than the dipole/dipole interactions among

ICl (97 C; molecular

similarly massed ICl molecules

mass 162 amu) and Br2 (59 C; molecular mass 160 amu) is __________.

Which one of the following should have the lowest boiling point? A) HCl B) H2S C) PH3 D) H2O E) SiH4

E. SiH4...