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33 Cards in this Set
- Front
- Back
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Metalloids |
more metallic physical properties nonmetal chemical properties |
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nuclear charge |
given by atomic number # protons for period trends inc → |
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effective nuclear charge |
charge based on attraction outer electrons feel (protons-inner electrons) created by shielding for periodic trends inc → |
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atomic radius |
-half the distance between 2 nuclei -increasesdown a group due to the increase of electron shells -decreasesdown a period because since they occupy the same energy level, the attractionbetween the nucleus and outer electrons increase and effective nuclear charge increases |
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ionic radius |
-positiveions are smaller than parents because they lose an outer shell -Negativeions are larger than parents because it adds electrons to the outer shell andthe increased electron repulsion causes them to move further apart -ionicradius decreases among positive ions due to the increase in nuclear charge which pulls the outer shell closer to thenucleus -ionicradius decreases among negative ions also due to increase of nuclear charge -Increasesdown a group as the number of electron energy levels increase |
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ionization energy |
-increasesacross a period because the increase in effective nuclear charge causes anincrease in the attraction between outer electrons and the nucleus and makesthe electrons more difficult to remove -decreasesdown a group because the effective nuclear charge is the same due to shieldingand the increased distance reduces the attraction between them |
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electron affinity |
-energychange when one mole of electrons is added to one mole of gaseous atoms -asthe added electrons are attracted to the positive nucleus, the process is anexothermic process -secondand third electron affinities are endothermic since electrons are repelled bythe negatively charged ion -likenegative first ionization energy |
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electronegativity |
-measureof the ability of its atoms to attract electrons in a covalent bond -increasesacross a period because the increase in nuclear charge resulting in anincreased attraction between the nucleus and the bond electrons -decreasesdown a group because electrons are furthest from the nucleus and so there isreduced attraction |
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melting and boiling points |
-Meltingpoints decrease down metallic groups because they are held together byattractive forces between delocalized outer electrons and this attractiondecreases with distance -meltingpoints increase down groups with nonmetals because the London dispersion forcesincreases as the number of electrons increases -meltingpoints across periods rise among metals to a max at 14 and decreases to a minat 18 due to the types of bonding |
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shielding |
minimizing of attraction between outer electrons and nucleus for group trends inc ↓ and attraction dec |
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energy levels |
size for group trends inc ↓ |
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isoelectronic |
same electron configuration for ion ans atoms |
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types of intramolecular bonding |
ionic and covalent |
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ionic |
metal + nonemtal electrons transferred 1 gains, 1 loses stronger bond due to electrostatic attraction checkerboard pattern for ions |
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covalent |
2 nonmetals shared electrons held by intermolecular forces (between molecules) -hydrogen (strongest), dispersion (weakest), and dipole-dipole (temporary electrostatic attraction) strongest covalent-giant molecular covalent (SiO₂) |
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group 1 properties |
physical good conductors of heat and electricity grey shiny surfaces when cut with a knife silvery metals chemical very reactive form ionic compound form single charged ions low ionization energies |
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group 2 properties |
physical shiny silver white metals good conductors high melting/boiling points chemical fairly reactive forms double charged ions forms ionic compounds |
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group 3 properties |
physical soft good conductors chemical somewhat reactive tends to form halides and oxides |
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lithium w/ water |
floats reacts slowly releases hydrogen keeps shape |
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sodium w/ water |
vigorous release of hydrogen heat produced melts metal small ball that moves around on the water's surface |
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potassium w/ water |
more vigorous release of hydrogen heat produced ignites hydrogen released lilac colored flame moves excitingly on water's surface |
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beryllium w/water |
does not react |
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magnesium w/ water |
reacts at boiling |
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group 2/ water |
reacts more vigorously with water as you go down group |
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period 3 oxides |
Na, Mg, Al- giant ionic P, S, Cl- molecular covalent Si- giant covalent ionic character is dependent on different electronegativity -decreases in period 3 oxides Na and Mg- basic (strength inc←) Al- amphoteric Si-Cl acidic (strength inc→) |
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formula for sodium oxide formula for sodium oxide w/ water |
4Na + O₂ → 2Na₂O Na₂O + H₂O → 2NaOH |
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formula for magnesium oxide
formula for magnesium oxide w/ water |
2Mg + O₂ → MgO₂ MgO + H₂O → Mg(OH)₂ |
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formula for aluminum oxide formula for aluminum oxide w/ water |
4Al + 3O₂ → 2Al₂O₃ Aluminum oxide doesn't dissolve in water but with acid and bases Al₂O₃ + 3H₂O + 2OH⁻ → 2Al(OH)₄ Al₂O₃ + 6H⁺ → 2Al³⁺ + 3H₂O Al₂O₃ + 3H₂SO₄ → Al(SO₄)₃ + 3H₂O |
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formula for silicon dioxide formula for silicon oxide w/ water |
Si + O₂ → SiO₂ does not react with water but reacts with bases to form silicates SiO₂ + 2OH⁻ → SiO₃²⁻ + H₂O |
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formula for the phosphorous oxide formula for the phosphorous oxide |
4P + 5O₂ → P₄O₁₀ 4P + 3O₂ → P₄O₆ P₄O₁₀ + 6H₂O → 4H₃PO₄ P₄O₆ + 6H₂O→ 4H₃PO₃ |
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formula for the chlorine oxide formula for the chlorine oxide |
2Cl₂ + 7O₂ → 2Cl₂O₇ (l) 2Cl₂ + O₂ → 2Cl₂O (g) Cl₂O₇ + H₂O → 2HClO₄ Cl₂O + H₂O → 2HClO |
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formula for the sulfur oxide formula for the sulfur oxide w/ water |
S + O₂ → SO₂ (g) 2S + 3O₂ → 2SO₃ (l) SO₃ + H₂O → H₂SO₄ SO₂ + H₂O → H₂SO₃ |
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other |
be able to explain periodic trends know different groups in the periodic table |
