Mr. Scharff. ShSht. Exam Review. Introduction to Chemistry

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1 Physical Science ShSht. Exam Review Name December 7, 2014 Pd. _ The pages that follow contain the many of the shortsheets that we completed collaboratively in class. I have given you these again to review and practice. Since, we completed all of these exclusively in class, you should have all of the answers in your science notebook in the shortsheet section to check as you complete any of the ones provided below. In addition to completion of these, you should know and understand all of your pregeame questions given in class each day, and you should know and understand all or your previous quiz questions. Any that you missed, I hope your corrected previously for partial points, but if not, you need to correct them know for understanding prior to the final examination. In addition, review the I can statements in your notebook for clarification. Good luck! If you need any help stop by and ask. Mr. Scharff Name Physical Science Date Pd. _ explain that atoms with the same number of positively charged protons and negatively charged electrons are electrically neutral. describe how ions are formed when an atom or group of atoms acquire an unbalanced charge by gaining or losing one or more electrons. ShSht. Charge Components - Student Directions. Refer to your class discussion notes and complete the miniaturized slide to the right of the table. Look at the example column in the table below and fill in the columns that follow. In the particle column indentify which type of subatomic particle, if any, should be used as this example. Example +1 Charge Value Charge Sign Charge Particle Side Bar: Understanding Atomic Charges of atom or subatomic particles (+/- #) of charge ( ) of charge ( or ) 26 Mr. Scharff Introduction to Chemistry Name Date Pd. Science Expectations (I can Statements) explain that atoms with the same number of positively charged protons and negatively charged electrons are electrically neutral describe how ions are formed when an atom or group of atoms acquire an unbalanced charge by gaining or losing one or more electrons Shsht. Number Sense of the Periodic Table A1 - student Directions. Complete the table below. You must show your work for any mathematical calculations. Atomic number = Mass number = Element Symbol Atomic number Atomic mass Number of protons Number of neutrons Number of electrons Scharffium 9 19

2 Introduction to Chemistry Name Date Pd. Science Expectations (I can Statements) explain that atoms with the same number of positively charged protons and negatively charged electrons are electrically neutral describe how ions are formed when an atom or group of atoms acquire an unbalanced charge by gaining or losing one or more electrons Shsht. Number Sense of the Periodic Table B1 - student Directions. Complete the table below. You must show your work for any mathematical calculations. Atomic number = Mass number = Substance Symbol Atomic Atomic Number of Number of Number of number mass protons neutrons electrons Colemanium Mr. Scharff Introduction to Chemistry Name Date Pd. Science Expectations (I can Statements) explain that atoms with the same number of positively charged protons and negatively charged electrons are electrically neutral describe how ions are formed when an atom or group of atoms acquire an unbalanced charge by gaining or losing one or more electrons Shsht. Number Sense of the Periodic Table C1 - student Directions. Complete the table below. You must show your work for any mathematical calculations. Atomic number = Mass number = Substance Symbol Atomic Atomic Number of Number of number mass protons neutrons Fremanigum-17 9 Number of electrons

3 Introduction to Chemistry Name Date Pd. Science Expectations (I can Statements) explain that atoms with the same number of positively charged protons and negatively charged electrons are electrically neutral describe how ions are formed when an atom or group of atoms acquire an unbalanced charge by gaining or losing one or more electrons Shsht. Number Sense of the Periodic Table D1 - student Directions. Complete the table below. You must show your work for any mathematical calculations. Atomic number = Mass number = Directions: Complete the columns on the table below. Consult your class notes as needed. You must show all mathematical calculations. Chemical Chemical Symbol Atomic Number Mass Number No. Protons No. Neutron No. Electrons Energy Levels # valence electrons Stable Ad If-41 20

4 On the back draw the atom and its energy levels with the correct number of electrons in each energy level.

5 Name Date Pd. Illustrate that atoms with the same number of positively charged protons and negatively charged electrons are electrically neutral demonstrate that when elements are listed in order according to the number of protons (called the atomic number), the repeating patterns of physical and chemical properties identify families of elements. Recognize that the Periodic Table was formed as a result of the repeating pattern of electrons. Shsht. Periodic Table Trends Try I Directions. Using the slides presented in our class discussion, answer the following questions regarding predictive patterns of elements on the periodic table. Draw in the stair-stepped line. A A 1. Which of the lettered elements is a gas? 2. Which of the lettered element represents a metalloid? 3. Which of the lettered elements has the largest diameter A, D D C C E E B B B, C, or D? 4. Which of these elements are transition metals? 5. What are the ionic charges of elements A, B, D? 6. What are the family names for elements A, B, D? Mr. Scharff Name Date Pd. Illustrate that atoms with the same number of positively charged protons and negatively charged electrons are electrically neutral demonstrate that when elements are listed in order according to the number of protons (called the atomic number), the repeating patterns of physical and chemical properties identify families of elements. Recognize that the Periodic Table was formed as a result of the repeating pattern of electrons.. Shsht. Periodic Table Trends Try II Directions. Using the slides presented in our class discussion, answer the following questions regarding predictive patterns of elements on the periodic table. Draw in the stair-stepped line. A 1. Which of the lettered elements is a gas? A 2. Which of the lettered element represents a metalloid? B C E F 3. Which of the lettered elements has the largest diameter? D 4. Which of these lettered elements are transition metals? D C B E 5. Which of these lettered elements have the same ionic I H charge? G 6. Which of these elements has the least ionization energy? J K 7. Which period has the greatest number of these elements? 8. Which of the following lettered elements has 0 valence electrons? 9. Which of the lettered elements has the largest charge value?

6 Name Date Pd. Illustrate that atoms with the same number of positively charged protons and negatively charged electrons are electrically neutral demonstrate that when elements are listed in order according to the number of protons (called the atomic number), the repeating patterns of physical and chemical properties identify families of elements. Recognize that the Periodic Table was formed as a result of the repeating pattern of electrons.. Shsht. Periodic Table Trends Try III Directions. Using the slides presented in our class discussion, answer the following questions regarding predictive patterns of elements on the periodic table. Draw in the stair-stepped line and number the periods on the left side of the periodic table. A A 1. How many energy levels in element A? 2. How many valence electrons in element A? 3. How many energy levels in element E? D D E C C E B B 4. How many valence electrons in element E? 5. What are the ionic charges of elements A, B, D? 6. Which of these elements has the greatest ionization energy? 7. How many other elements have the same number of valence electrons as element B?

7 Shsht. Electron Trends Take One Name Date Pd. _ A B Element A. Family? Number of energy levels? How many valence electrons? Reactive? Explain. How many additional electrons to become not reactive (stable)? Charge of this ion? Element B. Family? Number of energy levels? How many valence electrons? Reactive? Explain. How many additional electrons to become not reactive (stable)? Charge of this ion?

8 Shsht. Electron Trends Take Two Name Date Pd. _ D C Element C. Family Name Family Number Period Number Number of energy levels? Valence Electrons (Y/N) How many valence electrons? Reactive? Explain. Electrons gained/lost to become not reactive (stable)? How many? Charge of this ion? Element D. Family Name Family Number Period Number Number of energy levels? Valence Electrons (Y/N) How many valence electrons? Reactive? Explain. Electrons gained/lost to become not reactive (stable)? How many? Charge of this ion?

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10 Intro to Chem SS: The Lewis Electron-Dot Symbols of Elements I Name Date Pd. Directions: Complete the table according to each columns heading. Refer to your reading The Lewis Electron-Dot Symbols of Elements. Mr. Scharff sign: Element Chemical Symbol Electron Number Energy Levels (show number of electrons in each energy level present) Lewis Dot Diagram Calcium Flourine Mr. Scharff Intro to Chem SS: The Lewis Electron-Dot Symbols of Elements II Name Date Pd. Directions: Complete the table according to each columns heading. Refer to your reading The Lewis Electron-Dot Symbols of Elements. Mr. Scharff sign: Element Chemical Symbol Electron Number Energy Levels (show number of electrons in each energy level present) Lewis Dot Diagram Boron Argon

11 Science expectations (I can statements ) explain the relationship between molecular subscripts and coefficients ShSht: Chemical Numerical Notation Name Date Pd. Directions: Label the corresponding numerical parts of the chemical below. Complete the table by indicating the number of corresponding atoms for each element present in the chemical or sample. Numerical Parts of Chemical Chemical Sample C6H14N4O2 (Arginine) Kind and number of elements present Total number of atoms C8H9NO2 (Acetaminophen) Al(OH)3 (Aluminum Hydroxide) Mr. Scharff Name Date Pd. When observing chemicals, distinguish between atoms, elements, molecules and compounds ShSHt. Atom, Element, Molecule or Compound Take I Directions. Identify which term or terms from the title best describe the chemicals below. H 2 C 6H 12O 6 CO 2 Cl 2

12 Name Date Pd. When observing chemicals, distinguish between atoms, elements, molecules and compounds ShSHt. Atom, Element, Molecule or Compound Take II Directions. Identify which term or terms from the title best describe the chemicals below. CH 3COOH N 3 N 2 Cl-36 Mr. Scharff ShSht. Types of Bonding Hit it-one Name Date Pd._ Directions. Using your class materials, determine which type of bond is formed between the following elements and explain why this bond forms. 1. On the periodic table, what separates the metals from the non-metals? 2. What type of bond is formed between Chlorine atoms and Hydrogen atoms? Why: 3. What type of bond is formed between Oxygen atoms Chlorine and atoms? Why: 4. What type of bond is formed between Gold atoms and Gold atoms? Why:

13 ShSht. Types of Bonding Hit it-two Directions. Fill in the spaces on the table below based on our class discussion notes. 1. Will these chemicals form an ionic bond? Chemical Bond A: Magnesium and Chlorine Steps from notes Name Date Pd._ Result of step 2. Identify the cation and anion (on periodic table) 3. Write symbol of cation with its ionic charge, followed by the anion with its ionic charge 4. Balance the charges through subscript addition to each ion so the sum of the charges from each quantity of identical ions equals zero on the overall molecule for chemical formula 5. Write chemical name of the ionic compound and changing the last part of the anion name by adding the suffix ide Mr. Scharff ShSht. Ionic and Covalent Bonding Hit it-three Name Date Pd._ 1. An ionic bond forms between which periodic table elements? 2. A covalent bond forms between which periodic table elements? 3. A metallic bond forms between which periodic table elements? What is the chemical name of the compound made from the following elements ionic or covalent ionic or covalent ClO2 Ag2SO4 ionic or covalent Phosphorus Trioxide ionic or covalent ionic or covalent NF3 CaCl

14 Name Date Pd._ ShSht. Ionic and Covalent Bonding Hit it-four 1. A liquid substance has the ability to conduct electricity, and when cooled can be ductile and malleable, combines with a shiney, substance that has 2 valence electrons. What type of bond will form? 2. What type of bond will mercury and lead form? 3. What type of bond will Iron (III) and Oxygen form? 4. What will be the formula for Iron (III) and Oxygen? 5. What will be the name of Iron (III) and Oxygen? Mr. Scharff Intro to Chem Name Date Pd. explain the relationship between molecular subscripts and coefficients in chemicals and chemical reactions (e.g., writing correct chemical formulas and writing balanced chemical equations) ShSht. Ionization Compounds Go 1. Directions. Write the correct formula and name for the following ionization compounds. 1. Magnesium and Oxygen 2. Bromine and Calcium

15 Intro to Chem Name Date Pd. explain the relationship between molecular subscripts and coefficients in chemicals and chemical reactions (e.g., writing correct chemical formulas and writing balanced chemical equations) ShSht. Ionization Compounds Go 2. Directions. Write the correct formula and name for the following ionization compounds. 3. Hydroxide and Aluminum 4. Iron (III) and Oxygen Mr. Scharff Name Date Pd. _ explain the relationship between molecular subscripts and coefficients in chemicals and chemical reactions (e.g., writing correct chemical formulas and writing balanced chemical equations) ShSht. Balancing Equations A Directions. Construct a balancing table and balance the following chemical equations. Rewrite the equation balanced on the line below the balancing table. 1. MgCO3 MgO + CO2 2. Mg + N2 Mg3N2 Reactants Mg C O Products Mg C O Reactants Mg N Products Mg N

16 Name Date Pd. _ explain the relationship between molecular subscripts and coefficients in chemicals and chemical reactions (e.g., writing correct chemical formulas and writing balanced chemical equations) ShSht. Balancing Equations B Directions. Construct a balancing table and balance the following chemical equations. Rewrite the equation balanced on the line below the balancing table. 3. Zn + HCl ZnCl2 + H2 4. S8 + F2 SF6 Reactants Zn H Cl Products Zn H Cl Reactants S F Products S F Mr. Scharff Name Date Pd. _ explain the relationship between molecular subscripts and coefficients in chemicals and chemical reactions (e.g., writing correct chemical formulas and writing balanced chemical equations) ShSht. Balancing Equations C Directions. Construct a balancing table and balance the following chemical equations. Rewrite the equation balanced on the line below the balancing table. Hint make Hydrogen even number on products side first 5. K + H2O KOH + H2 6. Al + O2 Al2O3 Reactants K H O Products K H O Reactants Al O Products Al O

17 Name Date Pd. _ explain the relationship between molecular subscripts and coefficients in chemicals and chemical reactions (e.g., writing correct chemical formulas and writing balanced chemical equations) ShSht. Balancing Equations D Directions. Construct a balancing table and balance the following chemical equations. Rewrite the equation balanced on the line below the balancing table. 7. N2 + F2 NF3 8. S8 + O2 SO2 Reactants N F Products N F Reactants S O Products S O Mr. Scharff Name Date Pd. _ explain the relationship between molecular subscripts and coefficients in chemicals and chemical reactions (e.g., writing correct chemical formulas and writing balanced chemical equations) ShSht. Balancing Equations E Directions. Construct a balancing table and balance the following chemical equations. Rewrite the equation balanced on the line below the balancing table. 9. H2O + N2O3 HNO2 10. SnO + NF3 SnF2 + N2O3 Reactants H O N Products H O N Reactants Sn O N F Products Sn O N F

18 Phys Sci Name Date Pd. Shsht. States of Matter Atomic Structure student Directions. In the table below, make a diagram using 10 dots representing atoms or molecules indicating their placement in each of the three states of matter below. Label each state of matter and then explain 3 ways in which the states differ from each other. State of Matter: State of Matter: State of Matter: 1. Explanation Explanation Explanation

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