# IS 352 Test 1

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1. What are the 9 processes of Science?
• 1. Observing
• 2. Measuring
• 3. Classifying
• 4. Inferring
• 5. Predicting
• 6. Experimenting
• 7. Hypothesizing
• 8. Explaining
• 9. Communicating
2. Observing Activity
The candle was described qualitatively and quantitatively before it was lit, during burning and after burning.
3. Measuring Activity
Ice cubes were placed in a beaker. Observations were made and recorded. The height of the water in the beaker was measured before melting and after melting. The height did not change because the ice displaced the water and when it melted it filled the space up.
4. Classifying Activity
Buttons and "wild things" were classified as a binary classification system and a multi-stage classification system.
5. Inferring Activity
Why does moisture collect on a beaker of ice water? Because room temperature is warmer than the ice water and causes condensation. The condensation comes from the moisture in the air. We can show that the moisture does not come from inside the glass by adding food coloring to the water.
6. Hypothesizing Activity
The warmer water dissolved the Alka-Seltzer tablet faster than cooler water. The manipulated variable was the water temp., the responding variable was the time it took for the tablet to dissolve, and the control variables were the size of the tablet, the brand of the tablet, the water, the plastic cups, and the amount of water.
7. Predicting Activity
What's in a bag of M&M's? Predict the number of M&M's in a bag, the number of each color, and the most and least common colors. Compare data with the rest of the class groups and chart the data. On average there were more orange M&M's and the least amount were the red M&M's.
8. Communicating Activity
Tanagrams - one group member secretly made a design and tried to guide the other group members only with words on how to create the design. Not easy.
9. Matter
The stuff that everything is made of, or anything that has mass and volume
10. Mass
The amount of matter in an object, expressed in grams
11. Weight
The measure of the force exerted on an object by the pull of the Earth's gravity, expressed in Newtons
12. Volume
the amount of space taken up by an object, defined by l x w x h, or mL
13. Pure Substances
constant composition with a specific set of properties
14. Elements
basic building blocks of matter
15. Compound
2 or more elements
16. Mixtures
2 or more pure substances where each substance will keep its own identity, does not form a new substance. i.e. sweet tea
17. Difference between physical and chemical properties and change:
• Physical Properties - characteristics of an object that can be observed or measured, can be changed without changing the object itself
• Chemical Properties - chemical changes the ability of matter to change into a new substance that has different properties. i.e. sterling silver -> (oxidation) -> black color (petina)
18. 4 Signs that can tell you a Chemical Change has taken place:
• 1. gas is produced - fizzing
• 2. color change - rust
• 3. temperature change
• 4. produces light
19. Difference between heterogeneous and homogeneous mixtures:
• Homogeneous mixture - well mixed, appears to be uniform but proportions can vary. i.e. sugar in a glass of tea
• Heterogeneous mixture - not uniform, unevenly mixed
20. 3 Phases of Matter and difference in physical properties of each:
• Liquid - definite volume and indefinite shape
• Solid - definite volume and definite shape
• Gas - indefinite volume and indefinite shape
21. Burning a Candle Activity
The wick and wax work together as a system. The wax is the fuel and the wick transports the fuel to the flame. Without oxygen the flame cannot burn.
22. The Distinguishing Properties of Common White Powders
Each substance (granulate sugar, table salt, baking soda & cornstarch) behave differently when mixed with the various substances (water, iodine & vinegar). The biggest reaction came from mixing iodine with cornstarch. The cornstarch hardened and turned black. the other came when mixing vinegar and baking soda, which produces a gas evident from fizzing. Both of these are chemical reactions.
23. What are the properties of Oobleck?
Liquid or Solid? It doesn't have a definite shape, so it can't be a solid. It has a definite volume and no definite shape so it fits the definition of a liquid.
24. Changes of State of Water - 6 changes
• + Heat NRG
• Solid -> Liquid = Melting
• Liquid -> Gas = Evaporation
• Solid -> Gas = Sublimation
• - Heat NRG
• Gas -> Liquid = Condensation
• Liquid -> Solid = Freezing
• Gas -> Solid = Deposition
25. Latent Heat
The energy absorbed or released during a change of state.
26. Calories
the amount of heat it take to raise 1 gram of water 1 degree Celsius
27. Dew point temperature
the temperature at which the air must be cooled in order for condensation to occur
28. Condensation
change of state from a gas to a liquid with a loss of heat energy
29. Humidity
description of the amount of water vapor in the air
30. Saturation
the maximum possible amount of water vapor the air can hold at a given temperature and pressure
31. Meniscus
in a graduated cylinder the meniscus is read at the bottom of the curve
32. What is condensation and how does it occur?
Condensation is a change of state when a gas turns into a liquid with a loss of heat energy. The ice cools the sides of the cup which cools the warmer air that contains the water vapor very close to the outside of the cup. Water vapor gathers on the outside of the cup as condensation.
33. What is the temperature at which condensation takes place?
Condensation first started showing on the cup at 5 degrees Celsius, when the temperature had dropped 19 degrees.
34. 3 Subatomic Particles
• Proton - inside nucleus, + charge, atomic #, identification of element depends on the number of protons
• Electron - outside nucleus, - charge, # always = # protons, influence chemical reaction
• Neutron - inside nucleus, no charge
35. Atomic Number
the order of an element in Mendeleyev's table of the elements; equal to the number of protons in the nucleus
36. Atomic Mass Number (Atomic Weight)
Protons + Neutron = Atomic Mass
37. Molecule
2 or more atoms are combined, smallest unit of a compound
38. Organization of the Periodic Table - Names of Groups
• Rows: periods, there are 7
• Columns: family - there are 18, they react in the same way
• Group 1: Alkali Metal - very reactive, hardly find in nature
• Group 2: Alkaline Earth Metals
• Group 3 - 12: Transition Elements
• Group 13 - 16: BCNO
• Group 17: Halogens - non-metals, 5 elements, combine with alkali metals for form salts
• Group 18: Noble Gases - found in Earth's atmosphere, colorless and odorless
• Red Symbols: Gases
• Solid Black Symbols: Solids
• Blue Symbols: liquids at room temperature
• Outlined: Synthetic
39. Difference between a metal, nonmetal and metalloid:
• Metal (left hand side):
• Silver gray in color
• Malleable
• Shiny metallic luster
• Can be magnetic
• Good conductors of heat and electricity
• High densities
• Non-Metals (right hand side):
• Not shiny
• Transparent
• Brittle - will shatter
• Not magnetic
• Not conductors of heat or electricity
• Low density
• Some gases at room temp., some liquids & some solids
• Metalloid (semi-conductors in red outline):
• Solids
• Dull or shiny
• Malleable or brittle
• Density varies
• Conduct heat and electricity better than non-metals but not as good as metals
• Has properties of metal and non-metals
40. Which 2 elements are liquids at room temperature?
Bromine and mercury
41. Chemical bond
an attractive force that holds atoms together in a compound
42. Spheres of Hydration
The sphere of water molecules around each dissolved ion.
43. Cohesion
attraction of like molecules
attraction of dissimilar molecules
45. Chemical Reaction
a change in matter in which different chemical substances are created by breaking or forming chemical bonds
46. Hydrophilic
47. Hydrophobic
does not like water, i.e. oil
48. Endothermic
chemical reaction occurring or formed with absorption of heat
49. Exothermic
chemical reaction occurring or formed with the release of heat
50. 4 Types of Chemical Bonds
• Covalent - formed by sharing a pair of electrons, generally, non-metallic elements
• Polar - unequal sharing
• Non-polar - atoms share electrons equally
• Ionic - atoms transfer electrons, in general a metal reacts with 1 or more nonmetals
• Metallic - formed between 2 or more metals, give electrical conductivity
• Hydrogen - atoms share electrons in a water molecule
51. Unusual Properties of Water
• 1. The only substance found naturally on Earth in all 3 states
• 2. Temperature scales all based on water
• 3. Universal solvent
• 4. Density
• 5. Cohesion
• 6. Polarity of water - water attracts other polar molecules like sugar which is hydrophilic
52. Balance Chemical Equations
Practice
53. Law of Conservation of Mass
Matter is neither created nor destroyed during a chemical reaction
54. Oxidation-Reduction Reaction - Redox
An oxidizing chemical change where an element's electron loss is accompanied by a simultaneous electron gain.
55. Generalized form for Each of the Subclasses or Redox Reactions
• 1. Combination reaction: x + y -> xy
• 2. Decomposition reaction: xy -> x + y
• 3. Replacement reaction: xy + z -> xz + y
56. Chemical Heating Activity
The vinegar reacted with the steel wool and produced heat energy. Evidence of a chemical reaction: produced rust, heat, and moisture
57. Breakdown Activity
• Change hydrogen peroxide into water and oxygen with the aid of a potato
• Tiny bubbles form and rise to the top
• The potato releases oxygen to form bubbles
• Decomposition Reaction: H2O2 >> 2H2O(l) + O2 (g)
• The potato contains enzymes catalase that speeds up the reaction.
58. Exothermic Exercise
Mix yeast with hydrogen peroxide. The yeast reacted to the hydrogen peroxide and heat energy was released raising the temperature of the mixture. Evidence of a chemical reaction: heat is produced, bubbles produced
59. Endothermic Exercise
• The Epsom salt absorbed the water's natural heat energy to split apart the magnesium and sulphate therefore making the water cooler.
• MgSO4 + H2O
60. Bill Nye - Chemical Reactions
• Everything is mad of chemicals
• Chemicals react to make new chemicals
• Electrons hook together
• Chemicals react with chemicals in the air and give off heat
• Water is the most important chemical
• 92 pure elements
• Alfred Nobel - Swedish chemist who invented dynamite

## Card Set Information

 Author: kcooper ID: 71508 Filename: IS 352 Test 1 Updated: 2011-03-08 19:36:51 Tags: chemical bond matter mass weight periodic table Folders: Description: TAMU-Commerce IS 352 Test 1 Show Answers:

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