Alloys and Solids
What are the two types of alloy?
Interstitial
Substitutional
Put the following IMFs in order of increasing strength.
1. Hydrogen bonding
2. Ion-dipole
3. London dispersion
4. Dipole dipole
3<4<1<2
True or False: Particles in a solid are considered to be “mobile”
False
If something's randomness increased, but didn't have a major shift in volume, what phase change did it likely undergo?
Melting (solid to liquid)
What are the two parts of any solution?
Solute and Solvent
Must be similar in size
What is misleading about the term hydrogen bonding?
They aren't actual bonds.
What is it about the metallic solids that allows them to conduct electricity?
Sea of electrons (mobile electrons)
Is ice melting an exothermic or endothermic process?
Endothermic
Likes dissolves likes means...
Polar solutes can dissolve into polar solvents
Nonpolar solutes can dissolve into nonpolar solvents.
What type of alloy is represented here?
Substitional
What type of IMFs would be present between molecules of...
1. HCl and HF
2. H2 and HCl
1. Dipole-dipole
2. Dipole-Induced dipole
What is it about ionic compounds that does not allow them to conduct electricity as solids, but why can they conduct electricity when they're melted or dissolved?
* Solids -- Ions/electrons are not mobile
* Liquids/dissolved -- They are mobile
Is something dissolving a chemical reaction? Why?
Yes -- Bonds are being broken and IMFs are increased
No -- Bonds are broken, but bonds are not formed in a different way
What are at least three factors that impact solubility?
- Temperature
- Particle Size
- Polarity
- Pressure
What is another term for a network solid?
Can these conduct electricity?
What is an example of a network solid?
Giant molecule
Giant covalent molecule
** Not they cannot (because they're covalent)
*** Diamond, graphite, graphene, quartz
What explains the following trend in melting points?
H2 = -252.8˚C
HCl = -85˚C
HF = 19.5 ˚C
IMF strengths
** Be able to explain this in May
May style question - A sample of a hard, solid binary compound at room temperature did not conduct electricity as a pure solid but became highly conductive when dissolved in water. Which of the following types of interactions is most likely found between the particles in the substance?
A - Ionic bonds
B - Metallic Bonds
C - Covalent bonds
D - Hydrogen bonds
A
Which phase change causes the impact of IMFs to drastically change?
Melting
Freezing
Evaporating
Evaporating
Of the three solids listed, which would have the highest level of conductivity?
A. 0.1 M KCl
B. 0.1 M HCl
C. 0.1 M CH3OH
D. All have the same
** How do you know?
A --> Solution was made with an ionic solid
Copper and zinc have the same atomic radius. Which of the following best represents an alloy of these two metals?
** What type of alloy is this?
B -- Substitutional
Put the following compounds in order (from lowest to highest) based on their expected boiling points.
1. CH3CH2CH2CH2CH2CH2OH
2. CH4
3. NaCl
4. CH3CH2CH2OH
5. H2O
** Something for May
2 <4<1<5<3
The table shows the formulas and molar masses for three compounds. Which of the following is a list of the compounds in order of increasing boiling points?
A - Buatne < 1-propanol < acetone
B - Butane < acetone < 1-propanol
C - 1-propanol < acetone < butane
D - Acetone = butane < 1-propanol
B --> Ability to hydrogen bond
How can you determine a solution’s molarity if you are given its mass in grams and volume in milliliters?
1. Convert grams to moles
2. Convert mL to L
Divide 1 by 2