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CHEM EXAM 3
| what is the geometry of the structure when there is 2 effective pairs? | linear |
| what is the geometry of the structure when there is 3 effective pairs? | trigonal planar |
| what is the geometry of the structure when there is 4 effective pairs? | tetrahedral |
| what is the geometry of the structure when there is 5 effective pairs? | trigonal bipyramid |
| what is the geometry of the structure when there is 6 effective pairs? | octahedral |
| what is the shape and bond angle of the structure when there is 2 effective pairs and 0 lone pairs? | linear, 180 |
| what is key about the number of effective pairs and the lone electron pairs? | you count the one around the central atom |
| what is the shape and bond angle of the structure when there is 3 effective pairs and 0 lone pairs? | trigonal planar, 120 |
| what is the shape and bond angle of the structure when there is 3 effective pairs and 1 lone pair? | v-shape or bent, 120 |
| what is the shape and bond angle of the structure when there is 4 effective pairs and 0 lone pairs? | tetrahedral, 109.5 |
| what is the shape and bond angle of the structure when there is 4 effective pairs and 1 lone pairs? | trigonal pyramid, 107 |
| what is the shape and bond angle of the structure when there is 4 effective pairs and 2 lone pairs? | v-shape or bent, 104.5 |
| what is the shape and bond angle of the structure when there is 4 effective pairs and 3 lone pairs? | linear, 180 |
| what is the shape and bond angle of the structure when there is 5 effective pairs and 0 lone pairs? | trigonal bipyramid, 120, 90, 180 |
| what is the shape and bond angle of the structure when there is 5 effective pairs and 1 lone pairs? | see saw, 120, 90, 180 |
| what is the shape and bond angle of the structure when there is 5 effective pairs and 2 lone pairs? | t shape, 90, 180 |
| what is the shape and bond angle of the structure when there is 5 effective pairs and 3 lone pairs? | linear, 180 |
| what is the shape and bond angle of the structure when there is 6 effective pairs and 1 lone pairs? | square pyramid, 90, 180 |
| what is the shape and bond angle of the structure when there is 6 effective pairs and 0 lone pairs? | octahedral, 90, 180 |
| what is the shape and bond angle of the structure when there is 6 effective pairs and 2 lone pairs? | square planar, 90, 180 |
| what is endothermic? | when heat enters the system and the energy is taken from the surroundings so they are colder. And the system absorbs the heat/energy. |
| what is exothermic? | when heat leaves the system and energy is put out into the surroundings and the surroundings become hotter and the system releases energy/heat. |
| how do they products and reactants differ in a exothermic reaction? | in a exothermic reaction the products have less energy than the reactants. You have $20 → you give away $5 → now you have $15. Products have less because they lost energy to the surroundings. |
| how do they products and reactants differ in a endothermic reaction? | in a endothermic reaction the products have more energy than the reactants. You have $20 → you get $5 → now you have $25. Products have more because they gained energy from the surroundings. |
| what does less energy mean for stability. | less energy means more stable |
| what is atomic radius? | the size of an atom |
| what is the pattern of atomic radius across the periodic table? | AR decreases across the table because as you go more to the right were adding more protons which are strongly attracted to the electrons and so the protons pull the electrons tighter and closer which makes the atom smaller. |
| what is the pattern of atomic radius down the periodic table? | AR increases as you go down the table because the electrons spread out to more shells and so the atom gets bigger. |
| what is ionization energy? | the energy required to take away an electron from an atom. |
| what is the pattern of IE across the table? | IE increases as you go across the table because because since the atoms get smaller they have a tighter hold on their electrons so it requires more energy to take away an electron. |
| what is the pattern of IE down the table? | IE decreases as you go down the table because since the atoms are bigger the electrons are farther from the nucleus so you can easily take them away with little energy. |
| what is electronegativity? | the ability of an atom to attract a electron to itself. |
| what is the pattern of EN across the table? | EN increases across the table because there is more protons as you go to to the right and so those protons are so easily attracted to the electrons. |
| what is the pattern of EN down the table? | EN decreases as you go down because there is a weaker attraction when the atoms are bigger because the outer electrons feel less attraction, the atom isn’t as good at pulling electrons toward itself in a bond. because the electrons are so far away. |
| what is the overall pattern of AR, IE, EN? | IE and EN have the same pattern of increasing across and decreasing down and AR is the opposite. |
| what is a ionic bond vs covalent bond? | an ionic bond is between a metal and a nonmetal. covalent is between a nonmetal and nonmetal. |
| what is polar vs non polar? | polar is a bond when two elements unequally share an electron. non polar is when they share the election equally. |
| what is molecule polarity in lewis structures? | polar is a uneven/asymmetric election distribution and a asymmetric look visually. one side is more EN and it has a dipole moment. nonpolar is symmetrical. and it has a balanced EN and has no net dipole moment. |
| what is another term for polar? | "it has a dipole moment" |
| what does polarity depend on? | it depends on the atoms and how they're arranged. |
| what are some exceptions to the octet rule? | boron=only needs 6 electrons beryllium=only needs 4 |
| what is important to note about what elements can have an expanded octet? | only the 3rd row and lower can have expanded octets, which is more than 8 around the central atom. |
| what is key about the see saw shape? | see saw structures are always polar |
| what is the London dispersion forces? | the weakest force. ALL molecules have this force. |
| what is key about non polar molecules and LDFs? | for nonpolar molecules that is the only force they have. |
| explain London dispersion forces? | one side of a atom become temporarily more negative and so it pushes away the electrons in the atom next to it. and so the negative side of the first atom is attracted to the positive side on the other atom. |
| what is key about LDF and molar mass? | LDFs increase with atoms with a greater number of electrons or greater molar mass. |
| what are dipole-dipole forces? | the force that happens between separate polar molecules. |
| explain dipole dipole forces? | Molecules with permanent dipoles attract each other. The δ⁺ (positive) end of one molecule is attracted to the δ⁻ (negative) end of another molecule. |
| rank the forces from strongest to weakest? | ion-ion, hydrogen bonding, dipole dipole, London dispersion |
| rank the forces from weakest to strongest? | LDFs, dipole dipole, hydrogen bonding, ion-ion |
| what is hydrogen bonding? | direct H bond: H-N H-F H-O |
| what is ion ion bonding? | the strongest bond. between ionic compounds. metal and non metal. The cation and ion are attracted to each other. |
| what is key about a molecule that is polar regarding forces? | if a molecule polar it has London dispersion and dipole dipole. |
| what kind of forces does a nonpolar molecule have? | just London dispersion. |
| what is key about a molecule that has hydrogen bonding? | if it has hydrogen bonding then it had dipole dipole and London dispersion also. |
| explain boiling point and intermolecular forces? | the stronger the force, the higher the boiling point. because if it is a strong force then it will be harder to break down the bonds to turn it into a gas. |
| boiling point? | a high boiling point means it takes longer for it to boil and a low bp mean it doesn't take a long time for it to boil. |
| what are halogens? | F, Cl, Br, I, At, Ts |
| what are Nobel gases? | He, Ne, Ar, Kr, Xe, Rn, Og |
| what is also key about Nobel gases? | You use Nobel gases as a short cut for electron configuration. |
| bigger electrons mean bigger radius | true |
| how does solubility work? | polar dissolves polar things and nonpolar dissolves nonpolar. polar and nonpolar don't mix. |
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