History and Arrangement of the Periodic Table Unit 4 Day 1

Content Objective I CAN explain the historical development of the Periodic Table and use the Periodic Table to identify and explain the properties of chemical families, including alkali metals, alkaline earth metals, halogens, noble gases, and transition metals

Criteria for Success I CAN explain the contributions of Mendeleev and Mosley to development of the periodic table. I CAN explain how the Periodic Table was originally organized and compare the original organization to how it is organized today I CAN explain how the electron configurations of the elements contribute to their organization and properties on the periodic table

History of the Periodic Table A. Russian chemist, Dmitri ___________________, originally organized the periodic table by atomic _________. He was able to predict ________________________________ Mendeleev mass missing elements

History of the Periodic Table Moseley B. Henry _____________ helped to develop our modern periodic table arranged by atomic _________. mass

Introduction to Periodic Table A. Each square on the periodic table shows the name and basic information of one _________________. element

Introduction to Periodic Table B. The vertical columns of the periodic table are called _________, or ____________. 1. Each group contains elements with similar ________________________________ because they have the same number of ____________ electrons. C. The horizontal rows of elements in the periodic table are called ______________. groups families chemical properties valence periods

Types of Elements A. A ___________ is an element that is a _________ conductor of heat and electricity. 1. Most metals are also Lustrous _____________ and _____________ metal good Malleable ductile

Types of Elements Alkali 2. _____________ metals are the highly reactive metals in group 1A. a. Forms positively charged ions with _____ charge due to loss of 1 valence electron. b. Form ____________ by combining with oxygen. General formula is ______. Alkali +1 oxides X2O

Types of Elements c. Form ionic bonds with nonmetals, creating salts. d. Combine with OH- to form strong bases. General formula is X(OH). e. React violently in water to produce ___________ gas. hydrogen

Types of Elements Alkaline earth +2 oxides XO 3. _________________________ metals are the metals in group 2A. a. Forms positively charged ions with _____ charge due to loss of 2 valence electrons. b. Form ______________ by combining with oxygen. General formula is ______. +2 oxides XO

Types of Elements c. Form ionic bonds with nonmetals, creating salts. d. Combine with OH- to form strong bases. General formula is X(OH)2.

Types of Elements Transition 4. __________________ metals are between groups 2A and 3A. Transition

Types of Elements nonmetal poor B. A __________________ is an element that is, generally, a _________ conductor of heat and electricity. poor

Types of Elements brittle 1. Most non-metal solids tend to be _____________ rather than malleable and ductile. brittle

Types of Elements halogens noble gases 2. The Group 17 elements are also known as the _______________ and are extremely reactive. 3. The Group 18 elements are also known as the ____________________ and are relatively unreactive, or inert. halogens noble gases

Types of Elements metalloid C. A ________________ is classified as an element that has some characteristics of both metals and nonmetals. 1. Metalloids tend to be _____________________ of electricity. metalloid semiconductors

Types of Elements D. Seven elements on the periodic table exist in the ________________ state: H2, N2, O2, F2, Cl2, Br2, and I2. 1. Use the mnemonic: Have No Fear Of Ice Cold Beverages BrINClHOF diatomic

Alkali Metals Alkaline Earth Metals Metalloids Halogens Noble Gases Group # Ion formed Reactive? (to what?) Conductive? Lustrous? Malleable? Ductile?