Chemistry Chapter 7
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| Many properties of the atoms are due to what? | distance of the outer electrons from the nucleus, and the effective nuclear charge experienced by these electrons
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| What screen the outer electrons from the full charge of the nucleus? | core electrons
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| Do electrons in the same shell screen each other? | not effectively at all
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| What is the trend of effective nuclear charge as we move left to right across a period? | effective nuclear charge increases
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| What is the trend of atomic radii as we go down a column? left to right? | atomic radii increases as we go down a column and decreases as we go left to right
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| Are cations smaller or bigger than their parent atoms? | smaller
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| Are anions smaller or bigger than their parent atoms? | bigger
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| What is the size trend for ions of the same charge? | for ions of the same charge, size increases going down a column of the periodic table
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| Isoelectronic series | a series of ions that has the ame number of electrons. Size decreases with increasing nuclear charge as the electrons are attracted more strongly to the nucleus
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| ionization energy | the minimum energy needed to remove an electron from the atom in the gas phase, forming a cation.
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| second ionization energy | the energy needed to remove a second electron.
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| Why do ionization energies increase after all valence electrons have been removed? | because of much higher effective nuclear charge experienced by the core electrons.
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| What are the trend of ionization energy as we go down a column? left to right? | first ionization energy decrease as we go down a column and increases as we go left to right. The smaller atoms have a higher first ionization energy.
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| Electrons are first removed from where? | from the orbitals with the largest value of n
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| Electrons are first added to where? | to orbitals wtih the lowest value of n
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| electron affinity | energy change upon adding an electron to an atom in the gas phase, forming an anion.
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| What does a negative electron affinity mean? positive? | the anion is stable if it is negative. anion is not stable if it is positive.
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| What is the trend of electron affinities? | more negative as we go from left to right, little change as we go down column
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| What elements have the most negative electron affinities?? | the halogens
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| Is the electron affinities of the noble gases negative or positive? | all are positive
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| What is the trend in metallic character? | increases as we go down a column, and decreases as we go from left to right
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| characteristics of metals | good conductor of heat and electricity, luster, the metal atoms are oxidized to cations.
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| Metal oxides + acids --> ? | salts and water
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| are metal oxides basic or acidic? | basic
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| nonmetal characteristics | lack luster, poor conductor of heat and electricity, gases at room temperature. Compounds of entirely nonmetals are molecular. Form anions when they react wtih metals.
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| Are nonmetal oxides acidic or basic? | acidic
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| Nonmetal + bases --> ? | salt and water
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| Alkali metals | (group 1A), soft metals with low densities and low melting points. have the lowest ionization energies, so they are very reactive toward nonmetals. Form 1+ ions
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| Alkaline earth metals | (group 2A), harder and more dense and have higher melting points than the alkali metals. Very reactive toward nonmetals. Form 2+ ions.
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| Hydrogen | nonmetal, form molecular compounds w/other nonmetals, such as oxygen and halogens
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| Oxygen | (in group 6A), diatomic molecule, gain electrons from other elements, thus oxidizing them.
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| Ozone | O3
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| Halogens | (group 7A), nonmetals that exist as diatomic molecules, most negative affinities, form 1- ions.
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| Noble gases | (group 8A), monoatomic gases, unreactive because they have completely filled s and p subshells.
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| Do noble gases react at all? | only the heaviest noble gases are known to form compounds, and they do so only with very active nonmetals, like flourine
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