Chemical Bonds

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

16. Naming Ionic Compounds 1. MgF2 ___________________ 2. Rb2S ___________________ 3. Ba(NO3)2 ___________________ 4. (NH4)2Te ___________________ 5. (NH4)3PO4 ___________________ 6. Na2SO4 ___________________ 7. Cu3P ___________________________________ 8. Fe(OH)3 ________________________________ 9. Cr2(CO3)3 _______________________________________ 10. Sn(HCO3)4 __________________________________________

17. Metallic Bonds -like ionic compounds, metals in their ______ state form ________ structures -each metal atom contributes its _______ _________ to a ___________ _____ of electrons, which move freely throughout the solid -without its ________ _________, each metal atom forms a _________ _______ -the attraction between the ________ _________ and the _____________ ___________ is called a _________ _____ Properties of Metals -influenced strongly by the strength of attraction between the _______ ________ and the number of ____________ ___________

18. Properties of Metals A. Melting Point -since it doesn’t matter where the _________ _______ are within the _______ __________ of the metal, the cations _______ _________ easily, while still remaining in ______ _______ with each other, so ________ _______ temperatures are relatively ____ -the _________ the attraction between ________ ________ and the ____ of ______________ __________, the ________ the melting point temperature, so ________ atoms tend to have _______ melting point temperatures.

19. Properties of Metals A. Melting Point

20. Properties of Metals A. Melting Point -________ _______ temperatures are _________ by increasing the number of ________ ________ contributed to the _____ of ______________ __________. ___________ __________ like _______ and _________ contribute their ______ ________ electrons as well as their __________ __________ to the ____ of ________________ __________, __________ the melting point temperature dramatically.

21. Properties of Metals B. Malleability & Ductility -because particles in a metal can easily change position, they are __________, or can be __________ _____ _______ or other shapes easily -because particles in a metal can easily change position, they are __________, or can be __________ _____ _______ C. Durability & Boiling Point -even though particles in a metal can easily change position, they are __________ ____________, to the ____ of __________ surrounding them, and are __________ to _______ from the metal, giving them a high ___________ and a high ________ ______ temperature as well

22. Properties of Metals D. Conductivity -because __________ __________ in a metal are _____ ___ _____ while keeping _________ ______ intact, the __________ move _____ from place to place easily, so metal are _____ ___________ of _____ -because __________ __________ in a metal are _____ ___ _____, they move easily as a part of an ________ ________ when an __________ __________ or ________ is applied to the metal, and the ________ ________ structure of the __________ ________ allows the __________ to flow without _________ with the ________, which allows for little __________

23. Properties of Metals E. Luster -because ____________ ___________ are free to move, they can interact with ______, __________ and __________ ________ of _______, giving metals their _______ ________ F. Hardness & Strength -as the number of ___________ __________ contributed to the ____ of _________ increases, the strength of the _________ _____ increases, so metals such as _______, which contribute ____ ________, are relatively _____ and _____, while metals that contribute their outer __ electrons plus their inner __ electrons such as _________, _____, or _______ are relatively _____ and _______

24. Metal Alloys -because it doesn’t matter what _________ the _________ ________ are in in a metal, it is easy to introduce other _________ __________ into the ________ structure of a metal, creating an ______, or ________ of metals -in ______________ _______, atoms of one kind of metal, like _______, are replaced with atoms of another kind of metal, like _______, to form an ______ like ________ _______, which has the properties of both metals. Pure _____ is beautiful, rare, and almost completely _________, and so is highly valuable, but it is too _____ to be of much use by itself, so it is ________ with ________ and ______ to make _________ or _________ _____, which is still beautiful, but much _______ and _________ -in ______________ _______, atoms of another kind of element, like _______, are inserted into the spaces in between the cations of a metal like _____ to form _______ ______, which is _______, ________, and less ________ than _____