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Unit 4 Test Review
| Question | Answer |
|---|---|
| True or False. A crystal lattice is a three-dimensional structure formed by positive ions surrounded by negative ions and negative ions surrrounded by positive ions. | True |
| True or False. A sodium ion is more stable than a sodium atom. | True. Ions are more stable than atoms because they are closer to an octect. |
| True or False. In covalent compounds, atoms become chemically stable by sharing their valence elecetons. | True. Covalent compounds SHARE their valence electrons to equal out. |
| True or False. The oxidation number of a compound is equal to the number of valence electrons. | False. |
| The octect rule, states that, in chemical compounds, atoms tend to have... | The electrons configuration of a noble gas, or in other words, eight electons in the valence energy level. |
| Ionic Compounds have the net (overall) charge of... | 0, or neutral. |
| If a charge is negative, are any valence electrons transferred from the compound with the negative charge? | NO. It gains three, does not distribute it. |
| Physical Properties of a Ionic Compounds: (4) | 1. High melting/boiling point. 2. Good conductors under cetrain circumstances. (If solid, bonds are not broken and can not move 3. Solids at room tempeture 4. Very hard and brittle (so many layers in chrystal lattice) |
| _______ structures make up ionic compounds | Chyrstal |
| Electrostatic attraction basically means what...? | Opposite charges attract. |
| Lattice means...? | Overlapping |
| Definition: Energy released when seperate gaseous ions bond to form ionic solid. What is the term? | Lattice Energy |
| Released energy is....what type of energy? Negative or positive. | Negative. |
| The ______ (larger/smaller) amount of energy released, the stronger the bond is. | Larger |
| Why does the more energy released result in a stronger bond? | By losing energy, compounds become more stable. Therefore, making it stronger. |
| The more negative the lattice energy of an ionic compound is, the _______ (weaker/stronger) the bond is. | Stronger |
| What type of element does not have to form compounds? | Noble Gases because they have already obtained the octect rule. |
| If the electronegativity difference is between 0-0.4 it is ________ (nonpolar, polar, ionic) | Nonpolar |
| If the electronegativity difference is between 0.4-1.7 it is ________ (nonpolar, polar, ionic) | Polar |
| If the electronegativity difference is about 1.7 it is _________ (nonpolar, polar, ionic). | Ionic |
| If there is more than 1 valid way to create a Lewis Structure for the same compound, it is called a ________ structure. | Resonance (Structure) |
| Single bonds are the _________ (longest/shortest) and ___________ (strongest/weakest). | Single bonds are the LONGEST and WEAKEST. |
| In covalent bonding, can a bond ever share 1 electron? | NO. They form bonds in pairs of electrons. |
| If a compound is nonpolar, it shares electrons _________ (equally/unequally). | Equally |
| If a compound is polar, it share electrons __________ (equally/unequally) | Unequally |
| Ionic Compounds are between which two types of elements? Metal, nonmetals or metalloids. | Metals and Nonmetals |
| Covalent Compounds are between which two types of elements? Metal, nonmetals or metalloids. | Nonmetals and Metalloids. |
| Covalent Compounds have ____ (high or low) boiling and meltings point. | Low |
| Covalent compounds do NOT form ions. True or False. | True. |
| Covalent Compounds are good conductors. True or False. | False, Covalent Compounds are NOT good conductors. |
| Covalent compounds transfer and recieve electrons. True or False. | False, they SHARE electrons in bonds. |
| What type of compounds form formula units? | Ionic. |
| What type of compounds use prefixes in nomenclature? | Covalent. |
| What type of compounds form molecules? | Covalent. |
| Why is covalent compounds not good conductors? | In order to carry electric charge, you must have a charged particle to carry the charge but covalent does not have charged particles. |
| Metals are not necessarily the reason Ionic Compounds are good conductors. What's a difference in their properties? | Ionic Compounds are Brittle, Metals are bendable, shapeable and ductible. |
| Metals atoms replaced by others of similar size is called a what type of alloy? | Substitutional |
| Holes in the closest packed metal structures are occupied by small atoms called... | Interstititial Alloys |
| _______ compounds tend to form so that each atom, by sharing electrons, has an octet of electrons in its highest occupied energy level. | Covalent |
| Why is it some compounds are covalent or ionic? | Electronegativity difference! |
| • Type of bond depends on the elements differences in... | Electronegativities |
| The ______ (closer/further) the atoms are on the periodic table, the more evenly they share their electrons and therefore share their electrons and therefore more likely to form covalent bonds. | Closer |
| The _______ (closer/further) apart atoms are on the periodic table, the less evenly they share their electrons and therefore more likely to form ionic bonds. | Further |
| If there are two metals in the compound, it's most likely... | Ionic |
| If there are two of the same element, it is most likely... | nonpolar |
| If there are two different elements, but no metal, it is most likely... | Polar |
| A neutral group of atoms held together by covalent bonds vs. formula unit in ionic bonding is called? | Molecule |
| Molecular and Covalent Compounds are the same thing. True or False. | True. |
| The prefix 'hepta' means? | 7 |
| The prefix 'hexa' means? | 6 |
| The prefix 'tetra' means? | 4 |
| The prefix 'deco' means? | 10 |
| The prefix 'penta' means? | 5 |
| In Covalent Bondings _______ (never/always) use a prefix, unless it's mono in the first element. | Always, always, always! |
| Why no polyatomic in covalent naming? | Because they are ions and only participate in ionic bonding and have charges. |
| Why are there no prefixese in ionic bonding? | Ionic bonding relies on charges to equal to neutral. Not to form octects in different ways like covalent does. |
| H2O2 Exception of prefixes in Covalent | Hydrogen Peroxide |
| CH4 Exception of prefixes in Covalent | Methane |
| NH3 Exception of prefixes in Covalent | Ammonia |
| As you share ____ (more/less) bonds of electrons, length gets shorter and energy increases. | more |
| As you share more bonds of electons, length gets shorter and energy ________ (increases/decreases). | Increases. |
| The _____ (longer/shorter) the bond, the weaker it is. | Longer |
| The ______ (longer/shorter) the bond, the stronger it is. | Shorter |
| The same amount of energy must be used to break the bond and form neutral isolated atoms. True or False. | True. |
Created by:
lauraelzarad