Mrs. Hilliard
1. Valence electron 2. Period 3. Alkaline earth metal 4. Halogen 5. Metalloid 6. Hund s Rule 7. Representative element 8. Energy sublevel 9. Transition element 10. Electronegativity 11. Ion 12. Octet rule 13. Nuclear Fusion 14. Nuclear fission 15. Cation 16. Photon 17. Wavelength 18. Atomic Orbital 19. Noble Gas 20. Ground State 21. Principle Energy Level 22. Alkali Metal 23. Group 24. Pauli Exclusion Principle 25. Anion 26. Aufbau Principle
1. Valence electron- the electrons in an atom s outermost orbitals; determines the chemical properties of an element. 2. Period- a horizontal row of elements in the modern periodic table. 3. Alkaline earth metal- group 2 elements in the modern periodic table and are highly reactive. 4. Halogen- a highly reactive group 17 (7A) element. 5. Metalloid- an element that has physical and chemical properties of both metals and nonmetals. 6. Hund s Rule- states that single electrons with the same spin must occupy each equalenergy orbital before additional electrons with opposite spins can occupy the same orbitals. 7. Representative element- elements from groups 1, 2, and 13-18 in the modern periodic table. 8. Energy sublevel- the energy levels contained within a principle energy level. 9. Transition element- elements in groups 3-12 of the modern periodic table. 10. Electronegativity- indicates the relative ability of an element s atoms to attract electrons in a chemical bond. 11. Ion- an atom or bonded group of atoms with a positive or negative charge. 12. Octet rule- states that atoms lose, gain, or share electrons in order to acquire the stable electron configuration of a noble gas. 13. Nuclear Fusion- the process of binding smaller atomic nuclei into a single, larger, and more stable nucleus. 14. Nuclear fission- the splitting of a nucleus into smaller, more stable fragments, accompanied by a large release of energy.
15. Cation- An ion that has a positive charge. 16. Photon- A particle of electromagnetic radiation with no mass that carries a quantum of energy. 17. Wavelength- The shortest distance between equivalent points on a continuous wave. 18. Atomic Orbital- A three-dimensional region around the nucleus of an atom that describes an electron s probable location. 19. Noble Gas- An extremely unreactive group 18 element. 20. Ground State- The lowest allowable energy state of an atom. 21. Principal Energy Levels- The major energy levels of an atom. 22. Alkali Metal- Group 1 elements, except for hydrogen, they are reactive and usually exist as compounds with other elements. 23. Group- A vertical column of elements in the periodic table arranged in order of increasing atomic number, also called a family. 24. Pauli Exclusion Principle- States that a maximum of two electrons can occupy a single atomic orbital but only if the electrons have opposite spins. 25. Anion- An ion that has a negative charge. 26. Aufbau Principle- States that each electron occupies the lowest energy orbital available.
1. Which diagram correctly depicts the general trend in electronegativity? 2. Which diagram correctly depicts the general trend in first ionization energy? 3. Which diagram correctly depicts the general trend in ionic radius? 4. What is the energy required to remove an electron from an atom of an element in the gaseous state called? 5. What is the measure of the ability of an atom in a molecule to attract electrons to itself?
6. Which of the following elements is a metal? a. K b. C c. Si d. Ne 7. Which of the following elements is a metalloid? a. K b. C c. Si d. Ne 8. Which of the following elements is a non-metal? a. K b. C c. Si d. Te 9. What is the halogen that is in Period 3? 10.Which region contains the alkali metals? 11. Which region contains the noble gases? 12. Which scientist arranged the modern periodic table?
Element Block Characteristics A? Very Reactive, soft shiny metal B p Very electronegative, liquid at room temperature C d Liquid metal 13. What category of elements have the property of being malleable and ductile? 14. What category of elements have the property of being gases or dull solids and poor conductors of electricity? 15. Which block is element A most likely found in? 16. What is the most important characteristic in determining an element s chemical properties? 17. What do we know about elements in the same group?
B C 18. Which region is called the s-block on the diagram? 19. Which region is called the p-block on the diagram? 20. Which region is called the d-block on the diagram? 21. Which region is called the f-block on the diagram? 22. What will an atom that loses an electron form? 23. What will an atom that gains an electron form?
D B C A 24. Which label identifies the trough of the wave? 25. Which label identifies the crest of the wave? 26. Which label identifies the amplitude of the wave? 27. Which label identifies the wavelength of the wave?
28. Which element has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 8? 29. What is the electron configuration for the element Ruthenium (Ru)? 30. Which elements have 7 valence electrons? 31. What is the correct number of valence electrons in the element aluminum (Al)? 32. How many valence electrons does carbon (C) have? 33. How many valence electrons does oxygen (O) have?
34. What is the correct electron dot configuration (Lewis Dot Structure) for Germanium (Ge)? 35. What is the correct electron dot configuration (Lewis Dot Structure) for Phosphorus (P)? 36. What is the correct electron dot configuration (Lewis Dot Structure) for Chlorine (Cl)? 37. What type of orbital is shown in A? 38. What type of orbital is shown in B? 39. Which block contains 7 orbitals? 40. Which region contains elements with 6 valence electrons? 41. The octet rule states that atoms will electrons to achieve a complete set of eight valence electrons. A B
42. Which region contains elements with an electron configuration that ends with p1? 43. What is the noble gas configuration for barium (Ba)? 44. How many valence electrons are present in barium (Ba)? 45. What is the complete electron configuration for Ruthenium (Ru)? 46. What is the noble gas electron configuration for Selenium (Se)? 47. What is the correct electron dot diagram for Carbon (C)? A. B. C. D. 48. What is the period and group number of the element with the electron configuration of [Ne] 3s 2 3p 5?
49. What is the splitting of nuclei called? 50. What is the combining of nuclei called? 51.What is the correct orbital box diagram and electron configuration for Sulfur (S)? 52.What is the orbital box diagram and electron configuration for Iodine (I)? 53. What is the orbital box diagram and electron configuration for Selenium (Se)? 54. What is the maximum number of electrons that can occupy a single orbital according to the Pauli Exclusion Principle?
1. Endothermic reaction 2. Ionic compound 3. Formula unit 4. Metallic bond 5. Monatomic ion 6. Chemical Bond 7. Oxyanion 8. Polyatomic ion 9. Delocalized electron 10. Oxidation number 11. Electrolyte 12. Ionic bond 13. Covalent bond 14. Exothermic reaction 15. Polar covalent bond