Chapter 14
States of Matter
The video below explains the states of matter:
- Liquid - definite volume; assumes the shape of the container
- Solid - definite shape and volume
- Gas - no definite shape
The video below explains the states of matter:
Intermolecular and Intramolecular Forces:
This website explains intermolecular and intramolecular forces: http://huntinghills.rdpsd.ab.ca/docs/homework/intermolecular%20forces%20day%201.pdf
The video below further explains intermolecular and intramolecular forces:
- Intramolecular forces - covalent, ionic
- Intermolecular forces - dipole dipole (2 molecules; positive and negative attract); hydrogen bonding; london dispersion force
This website explains intermolecular and intramolecular forces: http://huntinghills.rdpsd.ab.ca/docs/homework/intermolecular%20forces%20day%201.pdf
The video below further explains intermolecular and intramolecular forces:
Heating and Cooling Curve:
heating curve - an upward pointing graph used to show the rise of temperature
This website explains the heating and cooling curve: http://www.kentchemistry.com/links/Matter/HeatingCurve.htm
heating curve - an upward pointing graph used to show the rise of temperature
This website explains the heating and cooling curve: http://www.kentchemistry.com/links/Matter/HeatingCurve.htm
Energy Requirement to change the states of matter:
heat of fusion - the energy used to melt one mole of a substance
heat of vaporization - the energy needed to change one mole of liquid to its vapor
Molar heat of fusion: H2O= 6.02 kJ/mol
Molar Heat of Vaporization: H2O = 40.6 kJ/mol
Activity: http://www.chemteam.info/Thermochem/Molar-Heat-Fusion.html
This website explains energy requirement to change the states of matter and includes a video that furhter explains it. Website/Video: https://www.khanacademy.org/science/chemistry/states-of-matter/v/change-of-state-example
This Calculation shows how to work an equation with the energy requirement to change the states of matter:
heat of fusion - the energy used to melt one mole of a substance
heat of vaporization - the energy needed to change one mole of liquid to its vapor
Molar heat of fusion: H2O= 6.02 kJ/mol
Molar Heat of Vaporization: H2O = 40.6 kJ/mol
Activity: http://www.chemteam.info/Thermochem/Molar-Heat-Fusion.html
This website explains energy requirement to change the states of matter and includes a video that furhter explains it. Website/Video: https://www.khanacademy.org/science/chemistry/states-of-matter/v/change-of-state-example
This Calculation shows how to work an equation with the energy requirement to change the states of matter:
Phase Changes: Evaporation:
-liquid to gas
-only occurs on surface
-temperature of any substance is related to the average kinetic energy of its particles
-some have low Kinetic Energy and some have high Kinetic Energy
-when the molecule leaves there is less energy in the system
-lower kinetic energy = lower temperature
-our sweat glands reduce our temperature
Condensation:
-gas to liquid
-KE and energy of attraction are about the same
-when gas molecules near the surface of a liquid are attracted to the liquid they strike and become part of the liquid's surface
-heating event
-steam burns worse than boiling water because there is more energy
-equal evaporation and condensation are the same volume and have the same temp.
-more evaporation than condensation = more gas less water; less volume; temp goes down
-more condensation than evaporation= increase volume; temp increase
Fog and Clouds:
-warm air rises and expands
-air expands and chills; the water molecules will slow down and stick together
-cloud and the fog form when lots of molecules stick together
Boiling:
-liquid to gas
-like evaporation
-temp a liquid will boil is a boiling point
-pressure affects the boiling point
-increase pressure= increase boiling point
-decrease pressure= decrease boiling point
-measured at standard pressure = 1 ATM
Freezing:
-when KE is lower and the energy of attraction is greater the liquid will freeze
-different liquids have different freezing points
This website explains phase changes. Website: http://www.chem4kids.com/files/matter_changes.html
The video below explains phase changes.
-liquid to gas
-only occurs on surface
-temperature of any substance is related to the average kinetic energy of its particles
-some have low Kinetic Energy and some have high Kinetic Energy
-when the molecule leaves there is less energy in the system
-lower kinetic energy = lower temperature
-our sweat glands reduce our temperature
Condensation:
-gas to liquid
-KE and energy of attraction are about the same
-when gas molecules near the surface of a liquid are attracted to the liquid they strike and become part of the liquid's surface
-heating event
-steam burns worse than boiling water because there is more energy
-equal evaporation and condensation are the same volume and have the same temp.
-more evaporation than condensation = more gas less water; less volume; temp goes down
-more condensation than evaporation= increase volume; temp increase
Fog and Clouds:
-warm air rises and expands
-air expands and chills; the water molecules will slow down and stick together
-cloud and the fog form when lots of molecules stick together
Boiling:
-liquid to gas
-like evaporation
-temp a liquid will boil is a boiling point
-pressure affects the boiling point
-increase pressure= increase boiling point
-decrease pressure= decrease boiling point
-measured at standard pressure = 1 ATM
Freezing:
-when KE is lower and the energy of attraction is greater the liquid will freeze
-different liquids have different freezing points
This website explains phase changes. Website: http://www.chem4kids.com/files/matter_changes.html
The video below explains phase changes.
Vapor Pressure:-in a sealed container a given amount of liquid in a container will decrease slightly
-eventually the volume will become constant
-the rate of evaporation and condensation will become constant
This website explains vapor pressure. Website: http://www.chem.purdue.edu/gchelp/liquids/vpress.html
The video below is a helpful video that explains vapor pressure:
-eventually the volume will become constant
-the rate of evaporation and condensation will become constant
This website explains vapor pressure. Website: http://www.chem.purdue.edu/gchelp/liquids/vpress.html
The video below is a helpful video that explains vapor pressure:
Different Types of SolidsCrystalline Solids:
1. ionic solids: ions; held by strong forces between opposite charged ions; stable
2. molecular solids: molecules; low melting temp because of intermolecular forces; relatively weak (non-polar)
3. atomic solids: atoms
Alloy:
-mix of 2 metals
-substitutional alloy (replace) ex:brass
-interstitial alloy (between; void areas) ex:steel
This website is a helpful link that explains the different types of solids. Website: http://misterguch.brinkster.net/typesofsolids.htm
Bonding in Solids
ionic solids:
-stable substances with high melting points, held together by strong forces
molecular solids:
-melt at low temp because they are easy to break
-dipole dipole hold solids together
-non-polar- london dispersion holds solid together
This website is a helpful link that explains the different types of bonds in solids. Website: http://chemed.chem.purdue.edu/genchem/topicreview/bp/materials/material1.html
1. ionic solids: ions; held by strong forces between opposite charged ions; stable
2. molecular solids: molecules; low melting temp because of intermolecular forces; relatively weak (non-polar)
3. atomic solids: atoms
Alloy:
-mix of 2 metals
-substitutional alloy (replace) ex:brass
-interstitial alloy (between; void areas) ex:steel
This website is a helpful link that explains the different types of solids. Website: http://misterguch.brinkster.net/typesofsolids.htm
Bonding in Solids
ionic solids:
-stable substances with high melting points, held together by strong forces
molecular solids:
-melt at low temp because they are easy to break
-dipole dipole hold solids together
-non-polar- london dispersion holds solid together
This website is a helpful link that explains the different types of bonds in solids. Website: http://chemed.chem.purdue.edu/genchem/topicreview/bp/materials/material1.html