3. Determine the total charge of an oxygen nucleus: Valence electrons are ELECTRONS on the outer most electron shell (principle energy level).

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1 Name: Period: Date: Hybrid Chemistry Regents Prep Ms. Hart/Mr. Kuhnau UNIT 2: Bonding Lesson 2.1: Ions and Ionic Bonding By the end of today, you will have an answer to: How do metals and non- metals bond to become stable? Do Now: 1. The atomic mass of titanium is atomic mass units. The atomic mass represents the (1) Total mass of all the protons and neutrons in an atom of Ti (2) Total mass of all the protons, neutrons, and electrons in an atom of Ti. (3) Weighted average mass of the most abundant isotope of Ti. (4) Weighted average mass of all the naturally occurring isotopes of Ti. 2. An electron in a sodium atom moves from the third shell to the fourth shell. This change is a result of the atom (1) Absorbing energy (2) Releasing energy (3) Gaining an electron (4) Losing an electron 3. Determine the total charge of an oxygen nucleus: Valence electrons are ELECTRONS on the outer most electron shell (principle energy level). A Lewis electron- dot diagram represents the number of VALENCE electrons 4. Draw a Lewis electron- dot diagram of calcium. The Octet Rule The electron configuration of EIGHT valence electrons is known as an OCTET. An octet represents the MAXIMUM number of valence electrons that an atom can have. Answer these questions: 5. Which elements have 8 valence electrons or a full octet in its outermost electron shell? 6. Which group are these atoms in? 7. What is this group called? The noble gases of group are very and undergo very few reactions. Chemical reactions occur when atoms try to achieve a full

2 NOTES: OCTET RULE IONS POLYATOMIC IONS IONIZATION ENERGY CALCULATING CHARGE IONIC RADIUS CRISS CROSS and REVERSE CRISS CROSS NAMING IONIC COMPOUND

3 Name: Period: Date: Hybrid Chemistry Regents Prep Ms. Hart/Mr. Kuhnau WORK #2.1: IONIC BONDING 20 points EXAMPLE: Element X reacts with chlorine to form an ionic compound that has the formula XCl2. To which group on the Periodic Table could element X belong? CLASS Example: A. Draw a Lewis dot diagram of Cl. Cl B. How many electrons does chlorine need to gain in order to achieve a full octet? C. How many electrons does chlorine need to lose in order to achieve a full octet? D. Would it be easier for chlorine to gain electrons to achieve a full octet or lose electrons to achieve a full octet? 1. What is the total number of electrons in a S 2- ion? (1) 10 (3) 16 (2) 14 (4) Compared to a calcium atom, the calcium ion Ca 2+ has (1) more protons (2) fewer protons (3) more electrons (4) fewer electrons 3. Which symbol represents a particle with a total of 10 electrons? (1) N (3) Al (2) N 3+ (4) Al Compared to an atom of phosphorus- 31, an atom of sulfur- 32 contains (1) One less neutron (3) one less proton (2) One more neutron (4) one more proton 5. When a lithium atom forms an Li + ion, the lithium atom (1) Gains a proton (3) gains an electron (2) Loses a proton (4) loses an electron 6. To form an ion, an atom of nitrogen will (1) Lose five electrons, and have a charge of - 5 (2) Lose five electrons, and have a charge of +5 (3) Gain three electrons, and have a charge of - 3 (4) Gain three electrons, and have a charge of When ionic bonds are formed, metallic atoms tend to (1) Lose electrons and become negative ions (2) Lose electrons and become positive ions (3) Gain electrons and become negative ions (4) Gain electrons and become positive ions 8. In which compound have electrons been transferred to the oxygen atom? (1) CO 2 (3) NO 2 (2) N 2O (4) Na 2O 9. Which formula represents an ionic compound? (1) NaCl (2) N 2O (3) HCl (4) H 2O 10. Which compound contains ionic bonds? (1) NO (2) NO 2 (3) CaO (4) CO Which elements combine by forming an ionic bond? (1) sodium and potassium (2) sodium and oxygen (3) carbon and oxygen (4) carbon and sulfur

4 12. What is the IUPAC name for the compound ZnO? (1) Zinc oxide (2) Zinc oxalate (3) Zinc peroxide (4) Zinc hydroxide 13. Which type of bond is formed when electrons are transferred from one atom to another? (1) covalent (2) ionic (3) hydrogen (4) metallic 14. The compound XCl is classified as ionic if X represents the element: (1) H (2) I (3) Rb (4) Br 15. A barium atom attains a stable electron configuration when it bonds with (1) one chlorine atom (2) two chlorine atoms (3) one sodium atom (4) two sodium atoms 16. What is the chemical formula of iron (III) sulfide? (1) FeS (2) Fe 2S 3 (3) FeSO 3 (4) Fe 2(SO 3) When ionic bonds are formed, metallic atoms tend to (1) lose electrons and become negative ions (2) lose electrons and become positive ions (3) gain electrons and become negative ions (4) gain electrons and become positive ions 18. Which formula represents lead (II) phosphate? (1) PbPO 4 (2) Pb 4PO 4 (3) Pb 3(PO 4) 2 (4) Pb 2(PO 4) 3 Answer questions 19 through 22 based on the information below. The atomic radius and the ionic radius for some Group 1 and some Group 17 elements are given in the tables below. 19. Estimate the radius of a Br ion. [1] pm 20. Explain, in terms of electron shells, why the radius of a K+ ion is greater than the radius of an Na+ ion. [1] 21. Write both the name and the charge of the particle that is gained by an F atom when the atom becomes an F ion. [1] Particle name: Charge: 22. State the relationship between atomic number and first ionization energy as the elements in Group 1 are considered in order of increasing atomic number. [1]

5 23. What is the total number of valence electrons in a sulfide ion in the ground state? (1) 8 (3) 16 (2) 2 (4) When a person perspires (sweats), the body loses many sodium ions and potassium ions. The evaporation of sweat cools the skin. After a strenuous workout, people often quench their thirst with sports drinks that contain NaCl and KCl. A single gram serving of one sports drink contains gram of sodium ions. In the space below, draw a Lewis electron- dot diagram for one of the positive ions lost by the body as a person perspires. 25. Which element forms a compound with chlorine with the general formula MCl? (1) Rb (3) Re (2) Ra (4) Rn 26. Explain, in terms of subatomic particles, why the radius of a chloride ion is larger than the radius of a chlorine atom. 27. Which changes occur as a cadmium atom, Cd, becomes a cadmium ion, Cd 2+? (1) The Cd atom gains two electrons and its radius decreases. (2) The Cd atom gains two electrons and its radius increases. (3) The Cd atom loses two electrons and its radius decreases. (4) The Cd atom loses two electrons and its radius increases. 28. What is the total number of electrons in a S 2- ion? (1) 10 (3) 16 (2) 14 (4) A metal, M, forms an oxide compound with the general formula M 2O. In which group on the Periodic Table could metal M be found? (1) Group 1 (3) Group 16 (2) Group 2 (4) Group Compared to a phosphorus atom, a P 3- ion has (1) more electrons and a larger radius (2) more electrons and a smaller radius (3) fewer electrons and a larger radius (4) fewer electrons and a smaller radius 31. Element X reacts with iron to form two different compounds with the formulas FeX and Fe 2X 3. To which group on the Periodic Table does element X belong? (1) Group 8 (3) Group 13 (2) Group 2 (4) Group When an atom of lithium loses an electron, the atom becomes a (1) negative ion with a radius smaller than the radius of the atom

6 (2) negative ion with a radius larger than the radius of the atom (3) positive ion with a radius smaller than the radius of the atom (4) positive ion with a radius larger than the radius of the atom 33. If an element, X, can form an oxide that has the formula X 2O 3, then element X would most likely be located on the Periodic Table in the same group as (1) Ba (3) In (2) Cd (4) Na 34. When sodium and fluorine combine to produce the compound NaF, the ions formed have the same electron configuration as atoms of (1) argon, only (2) neon, only (3) both argon and neon (4) neither argon nor neon 35. What can be concluded if an ion of an element is smaller than an atom of the same element? (1) The ion is negatively charged because it has fewer electrons than the atom. (2) The ion is negatively charged because it has more electrons than the atom. (3) The ion is positively charged because it has fewer electrons than the atom. (4) The ion is positively charged because it has more electrons than the atom. 36. A barium atom attains a stable electron configuration when it bonds with (1) one chlorine atom (2) two chlorine atoms (3) one sodium atom (4) two sodium atoms 37. The compound XCl is classified as ionic if X represents the element (1) H (3) Rb (2) I (4) Br 38. An atom of an element has a total of 12 electrons. An ion of the same element has a total of 10 electrons. Which statement describes the charge and radius of the ion? (1) The ion is positively charged and its radius is smaller than the radius of the atom. (2) The ion is positively charged and its radius is larger than the radius of the atom. (3) The ion is negatively charged and its radius is smaller than the radius of the atom. (4) The ion is negatively charged and its radius is larger than the radius of the atom. 39. As a chlorine atom becomes a negative ion, the atom (1) gains an electron and its radius increases (2) gains an electron and its radius decreases (3) loses an electron and its radius increases (4) loses an electron and its radius decreases 40. Which symbol represents a particle that has the same total number of electrons as S 2-? (1) O 2- (3) Se 2- (2) Si (4) Ar 41. Explain, in terms of electrons, why the bonding in NaCl is ionic. 42. In which compound is the ratio of metal ions to nonmetal ions 1 to 2? (1) calcium bromide (3) calcium phosphide (2) calcium oxide (4) calcium sulfide