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PBHS Chemistry I
Chapter 7 Ionic bonds & Compounds
| Question | Answer |
|---|---|
| elements found in groups 1A-7A are called ___________ | representative elements |
| _______________ are the electrons found in the highest occupied energy level of an atom | valence electrons |
| The ________ of valence electrons determines the chemical properties of the element | number |
| To find the number of valence electrons in an atom, simply look at its ________________ | group number |
| the elements in group 1A have ___ valence electron(s) | one |
| the elements in group 2A have ___ valence electron(s) | two |
| the elements in group 3A have ___ valence electron(s) | three |
| the elements in group 4A have ___ valence electron(s) | four |
| the elements in group 5A have ___ valence electron(s) | five |
| the elements in group 6A have ___ valence electron(s) | six |
| the elements in group 7A have ___ valence electron(s) | seven |
| the elements in group 8A have ___ valence electron(s) | eight |
| Valence electrons are usually the only electrons used in _____________ | chemical bonds |
| Electron dot structures (sometimes called ___________ Structures) | Lewis Dot |
| Electron dot structures are diagrams that show the valence electrons represented by ______ arranged around the chemical symbol | dots |
| _______, such as neon and argon, are unreactive… that is they are stable | noble gases |
| In 1916, Gilbert Lewis used the idea that noble gases were unreactive to come up with the ___________ | octet rule |
| In forming compounds, elements tend to want to achieve the electron configuration of a noble gas which has ________ electrons in its outer electron shell | eight |
| Recall that each noble gas has eight electrons in its highest energy level and a general electron configuration of _________ | ns2 np6 |
| Atoms of metallic elements tend to ___________ their electrons to get to the stable configuration of ns2 np6 | lose |
| Atoms of some non-metallic elements tend to ________ (ionic bond) or _______ (covalent bond) electrons to achieve an octet | gain or share |
| An atom starts ____________ because it has the same number of positive protons and negative electrons | electrically neutral |
| An atoms loss of valence electrons produces a ________ or a positively charged ion | cation |
| the gain of a negatively charged electron by a neutral atom produces an ___________ | anion |
| using a periodic table, p. 162 in your text, you can find that Beryllium (Be) has ____ valence electrons and most likely will have a _____ charge | two, +2 |
| using a periodic table, p. 162 in your text, you can find that Sulfur (S) has ____ valence electrons and most likely will have a _____ charge | six, -2 |
| Naming of ions Cations: use the ________ name of the element | unchanged |
| Naming of ions Anions: change the ending of the element name to _______ | -ide |
| Mixtures of two or more elements, one of which is a metal | alloy |
| common alloy mixing copper and tin | bronze |
| common alloy mixing iron and chromium | stainless steel |
| Metallic Bonds The valence electrons of a metal can be modeled as a _______… they are mobile and can drift freely from one part of the metal to another | sea of electrons |
| Metals are _________: they can be drawn into wires | ductile |
| Metals are ____________: able to be hammered or forced into shapes | malleable |
| The ___________ of an ion is the number of ions of opposite charge that surround an ion in a crystal | coordination number |
| Most ionic compounds are _____________ at room temperature | crystalline solids |
| Ionic compounds generally have ___________ melting points | high |
| Ionic compounds can conduct an ____________ when melted or dissolved in water | electric current |
| Lead(II) iodide (PbI2) or plumbous iodide is a _____________ at room temperature | yellow solid |
| Lead(II) iodide (PbI2) or ____________ is a bright yellow solid at room temperature | plumbous iodide |
| _______________ or plumbous iodide is a bright yellow solid at room temperature | Lead(II) iodide (PbI2) |
| Lead iodide is _________ due to its lead content. | toxic |
| In the nineteenth century Lead iodide was used as an artists' __________ under the name Iodine Yellow | pigment or paint |
| Lead iodide can be obtained as a yellow precipitate by reacting solutions of ___________ and sodium iodide | lead(II) nitrate |
| Lead iodide can be obtained as a yellow precipitate by reacting solutions of lead(II) nitrate and _________________ | sodium iodide |
| Lead iodide can be obtained as a ____________ by reacting solutions of lead(II) nitrate and sodium iodide | yellow precipitate |
| _____________ can be obtained as a yellow precipitate by reacting solutions of lead(II) nitrate and sodium iodide | lead iodide |
| Pb(NO3)2 (aq) + 2NaI (aq) → PbI2 (s) + 2NaNO3 (aq) is the ______________ for the reaction in our lab | chemical equation |
| in chemical formulas, always write the ___________ first | cation |
| in chemical formulas, the ___________ goes after the ion it affects and tells how many of that ion is in that compound and only goes on the chemical formula (not the name) | subscript |
| A ______________ is the lowest whole-number ratio of ions in an ionic compound | formula unit |
| Anions and cations have ____________ charges and attract each other by means of electrostatic forces | opposite |
| Anions and cations have opposite charges and attract each other by means of ________________ forces | electrostatic |
| electrostatic forces are called ______________ | ionic bonds |
| sodium (Na) has ________ valence electron and has a ________ charge; chlorine has _____ valence electrons and has a ______ charge; they form a compound with the formula _________ | 1, +1, 7, -1 NaCl |
| NaCl is called _____________ | Sodium Chloride |
| polyatomic ions are ions act as a single _______ with a charge over the whole ion | unit |
| SO4 is an example of a _____________ ion and has a charge of _____ | polyatomic, -2 |
| SO4 is called _____________ | sulfate |
| NH4 is called _______________ and has a charge of _______ | ammonium, +1 |
| the carbonate ion has a chemical formula of ________ and a charge of _______ | CO3, -2 |
| Al+3 + 3Br-1 forms ___________ | AlBr3 |
| Mg+2 ionically bonds with Cl-1 and forms a compound called ___________________ | magnesium chloride |
| : Mg+2 ionically bonds with Cl-1 and forms a compound called Magnesium Chloride; the formula unit ratio Magnesium to Chloride is 1:2, so the chemical formula is written __________ | MgCl2 |
| : Mg+2 ionically bonds with Cl-1 and forms a compound called Magnesium Chloride; the formula unit ratio Magnesium to Chloride is _________ so the chemical formula is written MgCl2 | 1:2 |
| Ionic compounds are electrically __________(the plusses and the minuses equal out) | neutral |
| more polyatomic fun: write the formula and charge for the hydroxide ion | OH, -1 |
| more polyatomic fun: write the formula and charge for the nitrate ion | NO3, -1 |
| write the compound name for Pb(NO3)2 | lead (II) nitrate |
| write the compound name for NH4OH | ammonium hydroxide |
| write the chemical formula for lead iodide | PbI2 |
| write the chemical formula for Iron(II)Oxide , Iron (III) Oxide | FeO, Fe2O3 |
Created by:
kcshiker
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