1 / 15

Chemical Bonds

Chemical Bonds. nucleus. Orbital Notation. Electron Configuration. Electron-Dot (Lewis-Dot) Structure. Chemical Bonds. +. proton. neutron. -. electron. nucleus. Orbital Notation. Electron Configuration. Electron-Dot (Lewis-Dot) Structure. Chemical Bonds. Name. Atomic Number. Be.

shaine-edwards
Download Presentation

Chemical Bonds

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemical Bonds nucleus Orbital Notation Electron Configuration Electron-Dot (Lewis-Dot) Structure

  2. Chemical Bonds + proton neutron - electron nucleus Orbital Notation Electron Configuration Electron-Dot (Lewis-Dot) Structure

  3. Chemical Bonds Name Atomic Number Be Symbol Atomic Mass + proton neutron - electron nucleus electron cloud Be Orbital Notation Be Electron Configuration Be Electron-Dot (Lewis-Dot) Structure

  4. Chemical Bonds Name Atomic Number O Symbol Atomic Mass + proton neutron - electron nucleus electron cloud O Orbital Notation O Electron Configuration O Electron-Dot (Lewis-Dot) Structure

  5. Draw orbital notations for the following: Draw electron configurations for the following: Draw electron-dot (Lewis-Dot) structures for the following: C C C Ne Ne Ne Mg Mg Mg P P P Ca Ca Ca

  6. Forming an Ionic Bond Na 1s 2s 2p Na Na 3s Cl Cl Cl 1s 2s 3s 2p 3p

  7. Forming an Ionic Bond Na 1s 2s 2p 3s 2s Na Na Cl Cl Cl 1s 2s 3s 2p 3p Be Be Be 1s O O O 1s 2s 2p

  8. Chemical Bond A. Ionic Bond

  9. A. Ionic Bond

  10. Properties of Ionic Compounds -when ionic compounds form, they form a _____________, a ________________ _________ arrangement of _______ and ________ ions -the energy required to separate _______ (6.02 x 1023) of ions from each other is called the ________________, the more ________ the lattice energy, the ______ the attraction between ions -the strength of the attraction between ions affects the compound’s __________ _________

  11. Properties of Ionic Compounds A. Lattice Energy

  12. Properties of Ionic Compounds A. Lattice Energy 0 -200 -400 F Cl -600 Br -800 I -1000 -1200 Li Na K

  13. Properties of Ionic Compounds A. Lattice Energy -the lattice energy is more negative in ionic compounds that have ____________________, because the ions are ___________________ to each other B. Melting and Boiling Points

  14. Properties of Ionic Compounds B. Melting and Boiling Points -ionic compounds with higher lattice energies have _________melting and boiling points temps. -smaller ions are more ________ attracted to each other, because the _______ is closer to the _______ _________, while ions with larger positive and negative charges are more ________ attracted to each other C. Electrical Conductivity -to conduct electricity, charged particles must be _________________, so ionic compounds generally do not conduct electricity as a _____, but generally do as a ______ or when ______________ _______________

  15. Properties of Ionic Compounds D. Hardness -the ions in ionic compounds with _______________ lattice energies are more _________ attracted to each other, so they tend to be ________ For Review 1. Rank the following ionic compounds, in order, from most negative to least negative lattice energy: RbCl, RbF, RbBr, RbI 2. Rank the following ionic compounds, in order, from highest to lowest melting point temperature: NaCl, MgCl2, MgO 3. Rank the following ionic compounds, in order, from softest to hardest: Li2O, Li2S, Li2Te, Li2Se 4. Rank the following ionic compounds, in order, from ions most strongly to ions least strongly attracted to each other: MgF2, RbCl, CaF2, CaCl2, MgO

More Related