CHEM 101 1st Edition Lecture 7Outline of Last Lecture I. Electron ConfigurationsII. The Periodic Table and Configurations III. Noble Gas ConfigurationsOutline of Current Lecture II. Regions of the Periodic tableIII. Covalent CompoundsCurrent LectureI. Regions of the Periodic tablea. The columns of the periodic table are known as ‘groups’ or ‘families’ and can be represented as G1, G2, G3… G18. The groups in bold are the ones you need to befamiliar withi. G1: the Alkali metals and Hydrogen. ii. G2: the Alkaline Earth Metals.iii. G3 through G12: the Transition Metals.iv. G13: B group (B= boron)v. G14: C group (C= carbon)vi. G15: N group (N= Nitrogen)vii. G16: O group (O= Oxygen)viii. G17:Halogens ix. G18:Noble Gases (aka: Rare Gases)b. The rows of the periodic table are known as ‘periods’: P1, P2, P3…P18These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.i. Any element on the periodic table can be describe by its group and period. c. Valence electrons (electrons located in the highest energy levels/ outer most orbitals) are found in the Main groups: G1, G2 (which compose the s-block) and G13-G18 (which make up the p-block). d. Elements from the f-block are highly unstable.e. All elements in the Halogens group have 7 valence electrons. II. Compoundsa. Covalent compounds: A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms. The stable balance of attractive and repulsive forces between atoms when they share electrons is known as covalent bonding.b. How do you know if you have a covalent bond? They won’t involve metals. Covalent bonds only occur among nonmetals. c. “Metals love their electrons so much they share but never lose them.”