PS+4+-+6th+Period+Brown

//-Balancing Ionic Bonds-// 1.chemical formula-like a word that stands for one type of chemical compound. 2.symbol- the letters that make up the compound.
 * Chemical Bonds**



3.subscript-the little numbers 4.oxidation number-the charge that results when the atom loses or gains electrons to become stable 5.bohr model- show the number of protons and neutrons as well as valence electrons and total electrons



6.ion-charged particles that has either more or fewer electron than protons



7.charge-positive negative or neutral 8.criss cross method-shows the charges of two elements and bonds them //-Chemical Bonding-// 9.valence electrons- electrons on the outer most ring of the atom



10.noble gases-more chemically stable than other elements because they have a complete outer energy level 11.stable- when an element has eight valence electrons on it's outer most shell 12.bond- what my baby and I share <3 13.Group 1,2,16,17-more stable than any other group 14.metals-metals tend to lose electrons to achieve a stable noble gas structure 15.nonmetals-tend to gain electrons ti achieve a stable noble gas structure 16.gain electrons- elements gain electrons to form ionic bonds 17.lose electrons-elements lose electrons to form ionic bonds 18.ionic bond-becomes stable through ionic bonds 19.covalent bond- becomes stable through convalent bonds //-Covalent Bonding-// 20.electrons-nonmetals tend to bond to become stable 21.covalent-to nonmetals bond 22.electron dot diagram- a way to represent an atom



23.paired electrons-electrons are groups of electrons on the top,bottom,left,right of the symbol of the atoms 24.unpaired electrons-electrons are electrons on the top,bottom,left,right of the symbol of the atom //-Ionic Bonding-// 25.ionic bond-bond between a metal and nonmetal 26.compounds-substances formed from two or more elements in which the exact combination and proportion of elements is always the same //-Physical and Chemical Changes-// //-Chemical Changes in Matter-// //-Energy&Chemical Reactions-// 27.energy changes-during a chemical reaction energy is used to break bonds,energy is released when new bonds are formed 28.exothermic reactions-reaction that releases energy 29.endothermic reaction-a change that releases heat 30.bonds breaking-when bonds break to become stable 31.bonds form-bonds from to become stable //-Chemical Reaction Types-// 32.chemical reaction-process in which one or more substances are changed into new substances 33.reaction-the substance that reacts 34.product-the new substance that is formed 35.synthesis-chemical reaction in which two or more substances combine to form a different substances 36.decomposition-chemical reaction in which one substance breaks down into two or more substances 37.combustion-a type of chemical reaction that occurs when a substance reacts with oxygen to produce energy in the form of heat and light
 * Chemical Reactions**



38.single replacement-chemical reaction in which one element replaces another element in a compound 39.displacement-distance and direction of an object's change in position from the starting point 40.double replacement-replacement that has two elements replaced in a compound 41. atoms rearrange- rearranging atoms so an equation is balanced 42. counting atoms- Counting the number of specific atoms of a certain element 43. subscript- shows how many atoms of a specific element there are 44. coefficent- number of compounds in an element 45. recognizing balanced equation- being able to recognize when an equation is balanced 46. reactants- the compounds on the left side of an equation 47. products- the compounds on the right side of the equation 48. acids- a substance with a Ph lower than 7 49. hydrogen ions- a hydrogen isotope with a - charge 50. hydronium- an acid compound 51. strong acid- an acid with a Ph much lower than 7 52. weak acid- an acid with a Ph around or a bit lower than 7 53. bases- a substance with a Ph higher than 7 54. hydroxide- a base compound 55. strong base- a base that is much higher than 7 56. weak base- a base that is around 7' 57. conductivity- the ease of flow of electrons through a substance 58. pH scale- determines if a substance is an acid or base



59. indicators- turns a slip of pH paper red or blue 60. neutralization- if a substance has a pH of 0


 * __Questions__**

1. Why does increasing the temperature speed up the rate of a chemical reaction? A. It allows for a higher concentration of reactants, providing more area for particle collisions to occur. C. Heating the reactants provides for fewer molecular collisions, increasing the rate if reaction D. It enables the reaction to proceed with less energy than initially required.
 * B. The average kinetic energy is increased, allowing more frequent particle collisions**.

2. There is scientific evidence of a person submerged in icy cold water and believed to have drowned, who was able to be revived without any signs of brain damage. There is further evidence of a person who was submerged in warm water for the same length as the other person but was not able to be revived. Which of the following best explain these phenomena? B. In warm water, the rates of the chemical reactions within the body are slowed down, causing death by drowning to occur more slowly. C. In icy cold water, the surface area of a body is larger because of the swelling caused by water consumption. This additional surface area protects the body, therefore preventing death or brain damage. D. In warm water, death by drowning occurs more quickly because the reactions of the bacterial substances within the water, which are not known to exist in icy water, affect the chemistry of a human body.
 * A. In icy cold water, the rates of chemical reactions within the body are slowed down. The brain does not use oxygen as fast; therefore, death or brain damage is prevented**.

3. For a laboratory experiment, students are reacting solid magnesium and oxygen gas to form solid magnesium oxide, as shown in the equation 2Mg(s) + O2 -> 2MgO(s). Students only have a limited amount of time for laboratory experiments. Which of the following ideas can a student implement to make the reaction occur quickly? A. Combine the solid and oxygen and place the contents in the refrigerator C. Combine the magnesium and the oxygen in a larger container than necessary D. Chop the solid magnesium into smaller pieces.
 * B. Reduce the amount of oxygen**

6. How many electrons must barium lose to achieve a noble gas electron configuration? A. 0 B. 1 D. 4
 * C. 2**

7. The arrangement of sodium ions and chloride ions in a crystal lattice of sodium chloride can be described as? B. A cluster of positive chloride ions and negative sodium ions in a specific pattern. C. A three-dimensional figure containing negative chloride ions and positive sodium ions in an alternating pattern. D. A two-dimensional figure containing negative chloride ions and positive sodium ions in a random pattern.
 * A. A three-dimensional figure consisting of a random pattern of negative chloride and positive sodium ions bonded together with ionic bonds.**

8. Which pairs of elements are most likely to form an ionic compound? B. F and Br C. Cs and Ar D. Al and I
 * A. Li and Cl**

9. Which of the following is NOT a characteristic of balancing a chemical equation? A. Atoms must always be conserved B. The formulas of the compounds can never be changed D. Atoms can always be rearranged
 * C. The relative number of reactants can never be changed**

10. What is the coefficient on Ag when the following equation is balanced? Ag(s) + H2S(g) -> Ag2S(s) + H2(g) B. 2 C. 4 D. 8
 * A. 1**

http://www.epa.gov/acidrain/education/site_students/phscale.html http://hyperphysics.phy-astr.gsu.edu/HBASE/CHEMICAL/acid.html http://www.iun.edu/~cpanhd/C101webnotes/chemical%20reactions/combustion.html http://www.skonline.org/courses/sci/SP111417000/Unit5/5-2ElectronDotDiagrams.htm http://www.ndt-ed.org/EducationResources/HighSchool/Electricity/valenceshell.htm
 * Helpful Websites**