Exam 1 review

Exam 1 review - Exam 1: Chapters 1, 2, and 13.6 1.1-1.2:...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Exam 1: Chapters 1, 2, and 13.6 1.1-1.2: Orbitals- Region of space that is occupied by an electron or a pair of electrons. Shells- Period number (1,2,3…) Subshells- s,p,d,f Orbital Orientation- s= circle, p= dumbbell Spin- up/down arrows representing electrons in their orbitals (↑↓) Electron Configurations Energy from low to high= 1s<2s<2p x =2p y =2p z <3s<3p<3d 2 electrons per orbital (↑↓) Hund’s Rule: Fill orbitals of equal energy with electrons in the same spin state until all the orbitals are half-full before continuing to fill. 1.3-1.5: Bonds and Lewis structures Bond Formation= H-H; H:H; H 2 Valence Shell: outermost shell Number of valence-shell electrons= group number in the periodic table Lewis Octet rule: All second period atoms pull to have 8 electrons in their valence shells Valence= Number of bonds formed for an atom to satisfy the octet rule Carbon needs 4 bonds! (Fluorine=1 bond; Nitrogen=3 bonds; Silicon=4 bonds) For most organic molecules, the number of bonds + the number of lone pairs= 4 pairs of electrons 1.6-1.8: Hibridization of Carbon Hybridization= mixing of valence-shell orbitals to give same number of hybridized atomic orbitals 1s2s2p sp 3 Sigma ( ơ ) bond: very strong, symmetrical, internuclear axis, always single bonds
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 3

Exam 1 review - Exam 1: Chapters 1, 2, and 13.6 1.1-1.2:...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online