Chem+Comm+Pd+2

=Unit 1 Review= Period 2 //**Chemistry**//


 * Water Use: //( Stephen Bart)//**

Concepts: Direct/Indirect
 * Direct- you can directly tell how much water you are using and can be measured for example- poring 1 gallon of water into a fish tank, or the bottles of water show exactly how much water is in each bottle.**


 * Indirect- you can’t really tell how much water you are using or even know you are using water to create a product. For example spraying down your car, using water to cut certain materials, using water to create electricity.**


 * Questions- how much water to make the egg? Water used to make wood for the coupe, how water was used to bring the egg to plate?**


 * Mixtures: (Homogeneous/Heterogeneous) (Andy, Doyle)**

Concepts: Definitions of each Examples of matter and classify each

Heterogeneous- (adj) composed of different substances or the same substance in different phases, as solid ice and liquid water.

Examples of heterogeneous matter: orange juice with pulp, concrete sidewalk

Homogeneous (adj)- is a substance or material that contains only one kind of compound or an element.

Examples of Homogeneous matter: jello, pudding, salt water, sugar, and pancake syrup.



Should be included: Diagram of the water cycle Each term and defined as needed
 * Water Cycle: (Brielle, Burns)**

- __Precipitation__: any form of water that falls (rain, sleet, snow, or hail)

- __Evaporation__: water converted from liquid to vapor

- __Transpiration__: moisture carried to plant roots.

- __Runoff__: movement from land to sea

- __Ground Water__: water held in underground soil or rock

- __Surface Water__: water on Earth’s surface

- __Aquifer__: a body of permeable rock that can contain or transmit groundwater.

- __Water table__ High = colder temperature Low = warmer temperature

- __Percolation__: movement and filtering of fluids

- __Condensation__: reverse of evaporation.


 * Ionic Compounds/Formula's (Kathleen, Brandon)**

Balancing Ionic Compounds - Balancing the quantity of each element so that the charge does not change. Balancing an equation means taking the charge of each compound and converting it to the other compound. Ex: Zn + HCl = ZnHCl

Cation – A positively charge ion. Ex: Ca-2

Anion- A negatively charged ion. Ex: OH- (hydroxide)

Naming Ionic Compounds- Most ionic compounds have two word names. First word is the name of the cation, and the second word is the name of the anion.

Example- NaCl 1) Find the cation and the anion: Na+ and Cl- 2) Find on periodic table: Sodium (Na+) and Chloride (Cl-) 3) Put together: Sodium Chloride

Concepts: Solubility of solids and liquids Graph Analysis Example questions
 * Solubility: (Jake, Alexis)**

Solubility- something dissolved in anything. Solubility in gases, low pressure= less soluble in liquid, high pressure= more soluble in liquid. Gases are usually more soluble at colder temperatures. Saturated solution- maximum quantity of solute is dissolved in a solvent. Unsaturated solution- less dissolved solute than the amount that it can normally hold at that temperature. Supersaturated- contains more solution then it can normally hold at that temp.
 * If you have 80g of KNO3 at 100 º C would it be saturated, unsaturated, or supersaturated?


 * In each solution is it saturated, supersaturated, or unsaturated?
 * 1) 100g of NANO3 at 35 º C
 * 2) 140g or KI at 15 º C


 * Density: (Lauren, Charlton)**

Formula D= M/V D= Density M- Mass V= Volume

1.) If 50 grams of a piece of metal displaces 5.59 ml of water when placed in a graduated cylinder, what is the density of the metal? What is the identity of the metal? D= 50 g/ 5.59 ml D= 8.94 g/cm3

Then metal found would be copper.

2.) What is the density of a substance that has a mass of 59 grams and a volume of 74 cm3? Will it float in water? D= 59 g/ 74 cm D= .797 = .80 D= .80 g/cm3

Yes, it will float because it is less than 1.0.

3.) What is the density of a substance that had a mass of 28 grams and a volume of 2.5 mL? Will it float in water? D= 28g/ 2.5 mL D= 11.2 g/cm3

No, it will sink because it is heavier than 1.0.


 * PH Scale and examples: (Moser, Courtney)**

//**Concepts: Diagram of scale-**// //**I****ons associated with acids and bases-**// pH focuses on concentrations of hydrogen ions (H+) and hydroxide ions (OH-).
 * Acid:** A solution that has an excess of H+ ions.
 * Base:** A solution that has an excess of OH- ions.

//**Examples of each-**// 0 - Hydrochloric Acid (HCl) 1.0 - Battery Acid (H2SO4 sulfuric acid) 2.0 - Lemon Juice 2.2 - Vinegar 3.0 - Apples 4.0 - Wine and Beer 4.5 - Tomatoes 6.6 - Milk
 * Acids **

7.0 - Pure Water
 * Neutral **

7.4 - Human Blood 8.3 - Baking Soda (Sodium Bicarbonate) 10.5 - Milk of Magnesia 11.0 - Ammonia 12.4 - Lime (Calcium Hydroxide) 13.0 - Lye 14.0 - Sodium Hydroxide (NaOH)
 * Bases **


 * Lead/Mercury (Ryder, Sammie)**

Information: Must give information for lead and Mercury (revert back to presentation notes) Mercury

Only metal in liquid form at room temperature Mercury in the air eventually settles into water or onto the land. A highly toxic form that builds up in fish, shellfish and animals that eat fish this is called Methylmercury.

Health effects: Exposeure at high levels can harm the brain heart kidneys, lungs and immune system of people of all ages. It has been demonstrated that high levels of methylmercury in the bloodstream of unborn babies and young children may harm the developing nervous system, making the child less able to think and learn.

What we are trying to do about it EPA issues regulations that require industry to reduce mercury releases to air and water and to properly treat and dispose of mercury wastes. EPA also works with industry to promote voluntary reductions in mercury use and releases, and with partners in state, local and tribal governments to improve their mercury reduction programs. EPA works with international organizations to prevent the release of mercury in other countries. The public can contribute to mercury reduction efforts by purchasing mercury-free products and correctly disposing of products that contain mercury by reducing demand for products whose production leads to the release of mercury into the environment.

LEAD

Lead was one of the earliest metals discovered by the human race and was in use by 3000 B.C

Lead is a toxic metal that was used for many years in paint and other products found in and around our homes.

Lead exposure can harm young children and babies even before they are born.

Our can get lead in your body by breathing or swallowing lead dust, or by eating soil or paint chips containing lead.

Lead poisoning occurs when lead builds up in the body, often over a period of months or years. The symptoms of lead poisoning may include:
 * Abdominal pain and cramping (usually the first sign of a high, toxic dose of lead poison)
 * Aggressive behavior

Reduced sensations
 * Constipation
 * Difficulty sleeping
 * Headaches
 * Irritability
 * Loss of previous developmental skills (in young children)
 * Low appetite and energy

Sources of lead poisoning
 * Paint
 * dust
 * soil
 * drinking water
 * Air


 * Water Purification: (Ricky, Kyle)**

Steps for Water Purification

Natural Water Purification
 * 1) Evaporation
 * 2) Bacterial Action
 * 3) Filtration

Purifying water through the Hydrologic Cycle

The sun provides energy for the water to evaporate. This resembles the process of distillation.

Evaporation leaves behind minerals, heavy metals, and other dissolved substances.

Water vapor condenses and falls as precipitation is made into raindrops and snowflakes are nature’s purest form of water containing only dissolved atmospheric gases.

However human activites release a number of gases into the air making today’s rain less pure than it used to be.

Bacterial Action

When raindrops strike the soil, they collect impurities.

But, as the water seeps through the ground the bacteria in the soil feed on those impurities and purify the water.

Filtration

As water seeps further into the ground, it passes through gravel, sand and rock.

This allows bacteria and suspended matter to be filtered out. Municipal Water Purification 1.Screening -Screening is a process of identifying apparently healthy people who may be at increased risk of a disease or condition. 2.Chlorination prior to another chemical Process 3.Flocculation- To precipitate 4.Settling- to place in a desired state or in order. 5. Removing large unwanted materials from water. 6. to introduce chlorine atoms into an organic compound by an addition or substitution reaction. 7.Optional Further Treatment- Aeration, pH adjustment ,Fluoridation




 * Water testing lab: (Aaron, Patrick)**

Data table: Calcium (Ca2+)


 * ** Solution ** || ** Observations (color, precipitate, etc…) ** || ** Result (Is ion present?) ** ||
 * ** Reference ** ||  ||   ||
 * ** Control ** || clear || no ||
 * ** Tap Water ** || clear || no ||
 * ** Natural Water from __ ** || clear || no ||

Data table: Iron (III) (Fe3+)


 * ** Solution ** || ** Observations (color, precipitate, etc…) ** || ** Result (Is ion present?) ** ||
 * ** Reference ** ||  ||   ||
 * ** Control ** || clear || no ||
 * ** Tap Water ** || clear || no ||
 * ** Natural Water from __ ** || clear || no ||

Data table: Chloride (Cl-)


 * ** Solution ** || ** Observations (color, precipitate, etc…) ** || ** Result (Is ion present?) ** ||
 * ** Reference ** ||  ||   ||
 * ** Control ** || white || yes ||
 * ** Tap Water ** || white || yes ||
 * ** Natural Water from __ ** || white || yes ||

Data table: Sulfate (SO42-)

From these results, a form of chloride could have been dumped in the brook somewhere upstream and it flowed downstream. In our tap water, chloride is also present. This shows that any substance can be in any kind of water and you don’t know what you’re drinking.
 * ** Solution ** || ** Observations (color, precipitate, etc…) ** || ** Result (Is ion present?) ** ||
 * ** Reference ** ||  ||   ||
 * ** Control ** || clear || no ||
 * ** Tap Water ** || clear || no ||
 * ** Natural Water from __ ** || clear || no ||

Water Softening Lab



In this lab we first filtered the water using sand. After the water was filtered with each different thing, we added 10 drops of sodium carbonate to one test tube and some ivory soap to the other. The ivory soap caused 1.5 inches of suds. Next we filtered the water using sand. A precipitate formed when sodium carbonate was added. The soap caused 3.5 inches of suds. Then we filtered the water using calgon. Sodium carbonate caused a reaction to this water too. There was only .3 inches of suds with this water. Last, we used the ion-exchange resin to filter the water. Sodium carbonate caused a precipitate when added to this. The ivory soap caused 2.5 inches of suds to form when added.