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NAME:________________________________DATE: _________________PERIOD:______ Compounds and Bonds Notes Compound Chemical Formula Subscript Coefficient Covalent Bond Metallic Bond Ionic Bond Molecule Polar Covalent Bond Nonpolar Covalent Bond Adhesion Cohesion Capillary Action Surface Tension Review of chapter 1: 1. The smallest particle of matter is an __________________. Different types of atoms make up _____________________, which are substances that cannot be broken down into simpler substances by ordinary chemical means. 2. Different elements can be found on ___________________________. 3. Atoms are made up of 3 sub-atomic particles called ________________, ___________________ and _________________. 4. Protons have a ____________________ charge and are located in the ________________ of an atom. 5. The number of protons is the ________________ ______________ on the periodic table 6. Neutrons have _________________________ and are also located in the ________________ of an atom. 7. Protons and neutrons make up an atoms _____________________. 8. An atoms mass = ___________________ + __________________. 9. The number of neutrons = _______________ - ________________. 10. Atoms are made up of mostly _______________ ______________. 11. Electrons fly around the nucleus in ___________________________, orbital’s and shells. 12. Na+ and Cl – are __________________; which are atoms with a positive or negative charge. 13. 18O and 16O are _____________________; which are atoms of the same type with a different mass. 14. ________________________ is the process by which the nucleus of an element releases energy and particles. 15. ________________________ elements can be helpful (treatments for cancers and diagnoses) and harmful in large amounts. 16. __________________ _______ is the amount of time it takes for the nuclei of an element to lose half its mass. Notes: 2.1 (pg 41-46) Elements combine to form compounds Compounds have different properties from the elements that make them I. A compound is a _______________________________________________ ___________________________________________________________ II. Compounds are different from mixtures because the elements that make up a compound are held together by _____________________ _________________. III. Properties of compounds are very different from the properties of elements that make them up. Atoms combine in predictable numbers IV. A Chemical compound is represented by a chemical ________________. a. For example H2O is the _____________ ____________ of water V. Each compound has a specific number of atoms of each element. a. For example H2O (water) contains ____Hydrogen atoms and ____ Oxygen atom. Total # of atoms =____+____ = ____ b. ________________________ - are numbers located in the bottom left side of an element. They tell the number of atoms present in the compound c. Coefficients - are numbers located in front of the compound, telling the number of compounds or molecules present i. For example: 2H2O = H2O + H2O (2 molecules of water) Coefficient Total # of Hydrogen = _____ x____ = _____ Total # of Oxygen = _____ x ______ = ____ Total # of Atoms = ______ + ______ = _____ Inventory Practice: determine how many atoms of each element are in each compound below and the total number of atoms in the compound. 1. HCl – chemical formula for hydrochloric acid 2. H2O2 – chemical formula for hydrogen peroxide 3. P3Br2 - chemical formula for triphosphorous dibromide 4. AgNO3 – silver nitrate 5. 2NaI – sodium iodide 6. 3CH4 - methane 7. 2Mg3(PO4)2 – magnesium phosphate 8. 4C4H8 – tertracarbon oxahydrate Review of 2.1 1. Compounds are different from mixtures because they are held together with ___________________ ____________________. 2. CO2 is an example of the ______________________ _____________________ of carbon dioxide. 3. The _______________________ in a chemical formula tells the number of atoms of that element present. 4. The _______________________in a chemical formula tells the number of compounds present. 5. How many atoms of each element are in carbon dioxide? What is the total number of atoms in 5CO2. COMPOUNDS: • Compounds are 2 or more elements held together with a _________________ _______________. • Properties of compounds depend on the elements that make them up and how those elements are _______________ to each other. These properties are usually very _____________________ from the individual elements that make them up. • The same elements can form different compounds with different properties: Example: _____________(water) – safe to drink, does kill bacteria _____________(hydrogen peroxide) – makes you vomit, used kill bacteria • Bonding occurs due to the fact that every atom wants to acquire: 8 __________________ _____________________ • ______________________ _____________________: are the electrons in the outer most energy level of an atom. (Farthest away from the nucleus). • A full valence shell requires _____ valence electrons. With the exception on Helium because helium 1st energy level is filled with only 2. Review: • Draw a Bohr model diagram of Helium-4 and label the valence electrons: 4 H P: M: E: N: # of Valence e-: Questions: does Helium-4 have a full valence shell? _______________________ • Draw a Bohr model diagram of Carbon-14 label the valence electrons: 14 C P: M: E: N: # of Valence e-: Questions: does carbon-14 have a full valence shell? _______________________ 2.2 Notes pgs 47-53 3 Main Types of Bonds: 1. ________________________ BOND: Bond between 2 ___________________. • Considered to be a “sea of electrons” with positive “islands” (nuclei) V Black = electrons, V= Valance electrons, Blue = protons Red = neutrons 2. ________________________ BOND: electrons are ____________________. • A bond between 2 ______________________________________. • 2 types of covalent bonds: ____________________________ and ________________________ 1. _____________________ ______________________: an equal sharing of electrons between atoms. Occurs between 2 atoms of the same element. 2. ___________________________: an _____________________ sharing of electrons between atoms. Occurs between 2 atoms from different elements Bond between two different types of atoms (elements) - Creating a slight negatively charged side and a slight positively charged side. - This polarity causes _________________________________, _______________________, ________________________ and __________________________, and allows plants move water up their stems for photosynthesis. - Cohesion - attraction between 2 ____________ molecules (2 of the same types of molecules sticking together) - Adhesion - attraction between 2 ____________ molecules (2 different types molecules sticking together) - Surface Tension- cohesive forces in water that cause it to bead and form a thin elastic film layer PENNY Capillary Action - ______________________________________________________ _______________________________. (Caused by the adhesion (attraction) of the water molecule to the side of the tube, and cohesion (attraction) between the water molecules. The water sticks together and pulls a trail of water up the tube (attraction) ) How water moves up a plant stem Chromatography 3. ___________________BOND: Bond between 2 oppositely charged ______________. • _________________________ are formed when atoms gain or lose electrons. When an atom loses an electron it has a ________________________ charge, and sometimes that “lost electron” is picked up by another element. The atom that picked up the lost electron, gains an electron becoming ________________________ charge. The positive ion is attracted to the negative ion forming an • An ionic bond occurs between a _________________ and a ___________________. • An electron is _________________________ from the metal, creating a positive charged ion called the ______________________. This transfer creates a negatively charged non-metal referred to as an ________________________. • The ___________________ ion is attracted to the __________________ ion, holding the two atoms together. • The positively charged ion can also be attracted to a positively charged molecule referred to as a __________________________________ ion. Which is basically a compound (molecule) with a positive or negative charge. Example: NaCl: Table Salt Metal(cation) = _____________, gives up an electron creating a _______________ ion Nonmetal (anion) = __________, accepts the electron creating a _______________ ion Positive and negative charges _______________________ each other, creating a bond holding the compound together. Review of 2.2 1. ________________ ________________ holds the atoms of a compound together. 2. The three major types of bonds are a. ___________________________ b. ___________________________ c. ___________________________ 3. ____________________ bonds form when an electron is transferred . 4. ____________________ bonds form when an electron is shared. 5. Ionic bonds form between 2 ___________________. 6. Covalent bonds form _____________________, and are created between 2 _______________________. 7. There are 2 types of covalent bonds ______________ and __________. 8. Covalent bonds form because of the _______________ Rule – which states that atom want to have _____ valence electrons (8). Notes: 2.3 (pgs 56-61) Substances’ Properties Depend on Their Bonds Metals have unique bonds I. Metal atoms share electrons in all directions with other metal atoms in a type of bond called a _____________________ ___________________. II. Metallic bonds are often referred to as a _________ of shared electrons. All the metal atoms ______________ their __________________electrons. Fixed (can’t move) Metal Ions Free electrons The metals are like “islands” in the sea of purple electrons III. Properties of metals are determined by the sharing of the electrons in the metallic bonds. The properties include ___________________, ___________________, and _________________________. Ionic and covalent bonds give compounds certain properties IV. Ions are tightly locked into place in the structure of a crystal, so ionic bonds are difficult to break. V. Ionic compounds generally have: a. High__________________________and ________________________ points b. __________________________ and ________________________ c. Do not _____________________________ electricity in solid form d. Break up into negative and positive ______________ when dissolved and will ______________________ an electric current in solution. ClSolid salt (NaCl) III. IV. Na+ Covalent compounds are not held together has tightly as ion. Covalent compounds tend to have: a. Low ____________________ and ____________________ points b. Molecules stay together when dissolved in water (do not separate like ions) c. A Covalent molecule’s ___________________ and __________________ affect their properties. i. For example – graphite, and diamond – both carbon compounds Covalent Compounds, Ionic Compounds, Metallic Compounds Covalent Ionic Metallic In solution: Dissolved salt Solid salt (NaCl) + Na sodium ion Clchlorine ion Bonding Graphic Organizer: