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Chemical Bonding

Transcript: What do you notice about the valence electrons? Are they balanced? 11/27/12 Warm-up: Describe one of the covalent bonding video from yesterday. Then cut out the Venn Diagram foldable and glue it into your IAN. Label one circle WATER BOND and the other METHANE/CARBON DIOXIDE BOND What are the charges of the two elements before bonding? Methane Bond Chemical Bonding Ionic Bond Carbon Dioxide Bond A non-metal and non-metal Electrons are shared between the elements. Exit Ticket: What are the differences between the two types of chemical bonds? What was an example of a chemical bond? 11/26/12 Warm-up: Review what are the two kinds of chemical bonds? Which element is the Cation? Which is the Anion? How do you know? Metals are either positively charged or negatively charged There are two types: Covalent and Ionic Exit Ticket: What is an Ionic bond and how is it different from a covalent bond? Covalent bond in Hydrogen Covalent bond in Water Calcium Chloride Ionic Bond Covalent Use your notebook foldables to take notes! Between a metal and non-metal Electrons are lost and gained or taken and given The non-metal gains (takes) the electron and the metal loses (gives) the electron Sodium Chloride bond Use the Venn Diagram foldable to compare and contrast the water bonds to the Methane and Carbon Dioxide Bonds Cations are positive and have more Protons Anions are negative and have more Electrons

Chemical Bonding

Transcript: Chemical Bonding By Dan Cody & Tim Lind HOW MANY BONDS ARE THERE!!!!!????? There are IONIC, METALLIC, NONPOLAR COVALENT and POLAR COVALENT BONDS. Ionic Bonds When an electron is transferred from one atom to another to make the bond. Always includes a metal and a non-metal can have single, double, or triple bonds. The more bonds, the stronger. Example: Taking candy from a baby... Covalent Bonds When the electrons are shared between atoms Polar When the atoms have equal electronegativity Example: A Smurf tug-of-war Non-Polar When one atom is stronger to have more of the electrons, but not enough to take them Metallic Bonds Bond between two or more metals in which the electrons are able to move freely. The results are usually malleable, ductile, along with other metallic properties example: Titanium Alloy. It's mostly titanium, but has a few other metals in the mixture. Iron Man's Suit is made of a type of titanium alloy

Chemical Bonding

Transcript: •Covalent Bonding- results from the sharing of electron pairs between two atoms •Types of Covalent Bonds- Polar-Covalent Bond- is a covalent bond in which the bonded atoms have an unequal attraction for the shared electron Nonpolar-Covalent Bond- a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge •Molecule: is a neutral group of atoms that are held together by covalent bonds Molecular Compund- is a chemical compound whoes smiplest units are molecules •Resonance Structure- is the structure of a bonded molecule that cannot be correctly represented by a singel Lewis Structure becuase is has more than one type of bond •Single Bonds- is a covalent bond in which one pair of electrons is shared between two atoms •Multipule Bonds- double and triple bonds Double Bond- is a covalent bond in which two pairs of electrons are shared between two atoms (stronger than signle bonds) Triple Bond- is a covalent bond in which three pairs of electrons are shared between two atoms (stronger that double bonds) •Ionic Compound- is composed of positive and negative ions that are combinded so that the numbers of positive and negative charges are equal •Formal Units-are the simplest collection of atoms from which an ionic compound's formula can be established •Properties of Ionic Bonds- Crystal Lattice-the symmetrical three-dimensional arrangement of atoms inside a ionic crystal Lattice Engery- is the energy released when one mole of an ionic crystalline compound is formed from gaseous ions • Metallic Bond- the chemical bonding that results from the attraction between metal atoms and the surrouding sea of electrons •Properties of Metallic Bonds- High electrical and thermal conductivity characteristics Strong absorbers and reflectors of light Higher energy levels Malleability- is the ability of a substance to be hammered or beaten into thin sheets Ductility- is the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire •Delocalized- electrons that do not belong to any one atom but move freely about the metal's network of empty atomic orbitals •Heat of Vaporization- is the heat absorbed by a unit mass of a material at its boiling point in order to convert the material into a gas at the same temperature Chemical Bonding Metallic Bonds •Properties of Covalent Bonds- Bond energy- is the energy required to break a chemical bond and form neutral isolated atoms Bond length- the average distance between two bonded atoms Ionic Bonds: Covalent Bonds

Chemical Bonding

Transcript: created by: Lizzie Belmar and Sarah Fenske Ex. When a hammer strikes metal, the ions move to new locations, but are still surrounded by electrons. Na + Cl --->Na Cl 2 3 a force that holds cations and anions together Naming transition metals: Write the metal's name without changes, but put a roman numeral behind it in parenthesis to show the charge, plus add -ide at the end of the nonmetal. (ex. 1) Cu O: copper (1) oxide (ex. 2) Ag O: silver (1) oxide single bond- 2 (cc) photo by jimmyharris on Flickr Naming with metals in groups 1-3: The metal is always first and the nonmetal is always last. The metal element has no changes, then the nonmetal with a suffix changed to -ide (ex. 1) KCl: potassium chloride (ex. 2) NaBr: sodium bromide 2 cation anion covalent bonding O + O ---> O O 2 H + H ---> H H Naming polyatomic ions: A group of atoms that has a positive or negative charge. Most polyatomic ions are anions. Just give a regular name to the compound without changes and no -ide (ex. 1) Mn(OH) : manganese (II) hydroxide (ex. 2) Rb (CrO ): rubidium chromate Naming covalent bonds: Put the metal first and indicate the number of atoms it has with a proper prefix. Then do the same with the other element. Change the ending to -ide on the second element and mono is ommited most of the time. (ex. 1) NF; nitrogen fluoride (ex. 2) Cl O; dichlorine oxide (ex. 3) N O ; dinitrogen trioxide The End (cc) photo by Metro Centric on Flickr N + N ---> N N 4 Salt(NaCl) (cc) photo by Metro Centric on Flickr 2 triple bond- a chemical bond in which atoms share elctrons to fill their outer energy level metallic bonding Ruby Ionic Bonding Lewis dot ex: Chemical bonding 2 + - attraction between metal cations and shared electrons that surround it double bond- 3 2 Al O 2

Chemical Bonding

Transcript: Conducts electricity Melting & boiling points vary Malleable (able to form shapes) N O N When determining the polarity of a molecule you base it off of the polarity of bonds and the shape of the molecule. Also, it depends on the electronegativity of the elements in the molecule. Electrnegativity is the ability of an element to attract electrons. 1.) Nonpolar covalent occurs when electrons are SHARED equally between the atoms Ex: H Properties: Bonding occurs to lower energy and have higher stablility. Electron-dot Structure Properties: Covalent Bonding Hard solids at room temperature Have high boiling & melting points Brittle Poorly conduct heat Can conduct electricity when dissolved in water or when the compound is melted N O Resonance structures are 2 or more electron-dot structures that can be written by placing a multiple bond between different atoms Sodium 2.) Polar Covalent occurs when electrons are shared UNEQUALLY between atoms Bonding 2 Na Ionic Bonding Occurs between 2 non-metals 2 atoms share electrons EX: OF, ClBr Molecule: group of elements bonded together by covalent bonds Electron-Dot for Covalent Compounds Ex: HBr H - Br Polarity Metallic Bonding Shows how the valence electrons are distributed Occurs between 2 metals Forces of attraction between free-floating valence electrons and positively charged metal atoms. Metals are made up of cations EX: Cu, Ti, Al 2 Soft solid at room temperature It has a low melting and boiling temperature Does not conduct electricity Non-Polar Covalent Polar Covalent Ionic Electron Dot example H - H The bonding occurs between a metal and non-metal. Ionic bonds are considered to be strong. Properties: H : H The anion and cation are strongly attracted to one another due to electrostatic forces Electrons are gained and lost during bonding Ionic compunds have formulas that indicate the # of atoms EX: CaCl

Chemical Bonding

Transcript: Bonds form definate shapes. Ionic Bonds Low Boiling Point Bond formed between a metal and a non-metal. Low Melting Point Solid at room temperature Covalent Bonds Bond formed between two non-metals. High melting point Bonds form no definate shape. High Boiling Point Ionic and Covalent Bonds Liquid or gas at room temperature

Chemical Bonding

Transcript: -occurs between 2 nonmetals -between a metalloid and a nonmetal -2 atoms share electrons -atoms share electrons Example: Example: -occurs between a nonmetal and a metal -valence electrons represented by dots placed around the chemical symbol -electrons placed up to 2 on each side of symbol up to a maximum of eight -place a single electron on each side before pairing -period one has exception, only maximum of 2 electrons are placed on 1 side of element -high melting points -positively charged metal ions Electron-dot structures -usually liquids or gases at room temperature A force of attraction that holds atoms or ions together in a molecule or crystal. Bonds are usually created by a transfer or sharing of one or more electrons. There are single, double, and triple bonds. By: Joanna Josten polarity refers to a separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multipole moment. Polar molecules interact through dipole–dipole intermolecular forces and hydrogen bonds. Molecular polarity is dependent on the difference in electronegativity between atoms in a compound and the asymmetry of the compound's structure -without bonding, the universe would be nothing more than a mass chaos of individual atoms. -binds oppositely charged ions using electrostatic force of attraction -ionic compounds are electrically neutral -occurs between free-floating valence electrons Chemical Bonding! Properties: Bonding: Example: Why is bonding important? -when dissolved in water or melted, ionic compounds conduct electricity -solids at room temperature Properties: Polarity Covalent Bonding 3 main types of bonding: Properties: Metallic Bonding Ionic Bonding -conductive -bond occurs between 1 or more metals

Chemical Bonding

Transcript: . Ionic . (molecules) - . Nonpolar molecules: contain one nonpolar bond, or are symmetrical in electron dot formula, with no lone pairs areund central atom Ionic: Metal+Nonmetal, Conducts electricity (when melted), high meltin/boiling points, soluble in water . the shape of a molecule and the polarity of its bonds determine the polarity of the molecule (306 Basic Chemistry) . . Nonpolar Covalant Bond: When electrons are shared similarily, and pretty equally in a covalant bond . . Polar molecule: Unbalanced negativity, depends on shape of electron groups around central atom, dipoles dont cancel each other out. . Polar Covalant Bond: When electrons are shared unevenly in a covalant bond . . . 2 Definition: Show how the valance electrons are distubted Examples: P B Why so important? Bonding keeps atoms together, therefore, allowing the universe to work properly. With out bonding, the world would be a mass of individual atoms floating out and about. Try Chemical Bonding with electron dots: CCl 18e- 1.) Find the number of valance electrons Cl-C-Cl 14e- 2.) Use the central atom in the middle, and subtract two electrons from each bond (one line= 2 electrons) Cl-C-Cl 3.) Distribute the rest of the electrons; if needed, use double or triple bonds to compensate Types . . . . Chemical Bonding: keeps atoms together in strong attractive forces. . definition- A measure of unequal sharing of electrons, indicated by the difference in electronegativity values (304 Basic Chemistry) Bonding CHEMICAL BONDS BY: Sara Lawler . . . Properties . Covalant Polarity Metallic: 2 Metals (or including a metalloid), Malleable, various melting points, good conductors Covalant: 2 Nonmetals, poor conductors of electricity, low melting/boiling points, soluble in nonpolar liquids Electron-Dot Structures: The three main types of bonding are: . (bonds) Metallic

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