STM128

• Intermolecular forces are attractive forces between atoms/molecules, and these become stronger as the particles move closer together.
• Motivators and hindrances in getting to know strangers and mingling into a crowd can vary depending on the individual.
• Computing for the concentration of solutions can be challenging due to factors such as impurities, temperature, and pH.
• Physical properties of solutions are important for various reasons, such as understanding the solubility of substances, predicting the behavior of solutions, and designing experiments.
• In a room filled with people whom you just met, it can be challenging to find yourself.
• The molality of an alloy containing 0.025 g of silver and 3.95 g of iron is not known.
• People also have factors that affect their ability to get to know others and mingle into a crowd, which can be compared to how substances dissolve in other substances.
• Answers must be written with the correct number of significant figures and proper units.
• The percent by volume of ethanol (C 2 H 6 O) in a solution that contains 65.0 mL of ethanol dissolved in 355 mL of water (H 2 O) is not known.
• From what have you learned in this lesson, what recommendations can you give for future reference?
• Written Work (25 Points)
• Physical properties are affected by the strength of intermolecular forces.
• Intermolecular forces are the forces that bind two molecules together.
• Performance Task Laboratory Report: Viscosity
• Developed by Anita R Tagadia 2000
• As a Grade 12 student who will be graduating soon, how often do you bond with your friends and classmates? Do you think physical bond creates more memories than virtual interactions? Why or why not?
• In life, we create bonds with other people and our physical bond determines how strong the attraction we have for other people such as our friends, family, and loved ones.
• Note: Please refer to the rubric for the criteria on timeliness.
• The goal of the laboratory report is to compare the viscosity of water and corn syrup and determine the effect of temperature on the viscosity of honey.
• The role of a senior high school student in the laboratory report is to verify what they have learned in the classroom about viscosity.
• If the laboratory report is submitted 1 week after the due date, the highest possible score of the group will be determined by the lowest score from the groups who submitted on time.
• The temperature dependence of the solubility of some ionic compounds in water shows that in most cases, the solubility of a solid substance increases with temperature.
• The concentration of a solution is a measure of how much solute is dissolved in a specific amount of solvent or solution.
• A solubility curve is a data-based graph comparing the amount of solute that will dissolve in a given amount of solvent at various temperatures.
• Breaking the solute into small pieces increases its surface area, allowing more collisions to occur.
• The lines on the solubility curve indicate a saturated solution, a solution that has the maximum amount of solute dissolved in 100 g of water.
• Agitation is the stirring or shaking of a mixture, which moves dissolved solute particles away from the contact surfaces more quickly and allows new collisions between solute and solvent particles to occur.
• A concentrated solution contains a large amount of solute, while a dilute solution contains a small amount of solute.
• The lighter tea is dilute and contains less tea particles than the darker tea.
• Any amount below the line for a particular substance shows an unsaturated solution, and anything above the line shows a supersaturated solution.
• Solutions are often described quantitatively, expressing concentration as a ratio of measured amounts of solute and solvent or solution.
• The darker tea has more tea particles than the lighter tea, indicating that it is more concentrated.
• A teaspoon of granulated sugar dissolves more quickly than an equal amount of sugar in cube form.
• Concentration can be described qualitatively using the words concentrated or dilute.
• Being composed of atoms rather than ions, network solids do not conduct electricity in any state.
• Sodium Chloride (NaCl) Crystal, an Ionic Solid
• Molecular (polar or non-polar) solids are solids whose composite units are molecules and are held together by intermolecular forces (dispersion forces, dipole-dipole forces, and hydrogen bonding).
• These delocalized electrons do not belong to any one atom, but are capable of moving through the entire crystal.
• The states or phases of matter include solid, liquid, and gas.
• Metals are good conductors of electricity due to these delocalized electrons.