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26 Cards in this Set
- Front
- Back
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How to determine # of valence electrons?
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by group. pay attention to superscripts of + (meaning less electron, and - meaning more electron)
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how to determine which subshell will have the lowest efficiency for screening of nuclear charge?
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subshell farthest from the nucleus is least efficient at screening nuclear charge.
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how to find the most common metal ion?
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metals lose electrons to get the same number of electrons as the nearest noble gas
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how to find the most common non-metal ion?
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nonmetals gain electrons to get the same number of electrons as the nearest noble gas
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how to find the smallest atomic radius?
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radius gets smaller across the period, larger down the group
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how to find the largest atomic radius?
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radius gets smaller across the period and larger down the group
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what is isoelectronic?
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having the same number of electrons. can apply to an element, ion, or compound. just find the total number of electrons and compare.
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how to find the smallest radius in a group of ions?
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in groups of ions with the same # of electrons,
negative ion = largest most positive ion = smallest remember, radius gets smaller across the period, and larger down the group |
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what does I₁ mean?
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ionization energy
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how to find the ionization energy (I₁)?
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ionization energy increases across the period and up the group.
comparable to electronegativity- highest in the top right corner. |
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how to find which has NO non-binding electrons on the central atom?
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write a lewis structure
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how to determine if a compound is electron deficient?
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look for an empty orbital, which means it is electron deficient (look for the element without an octet)
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how to determine if there is NO double bond present in a compound?
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make a lewis structure
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what is an expanded octet?
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an element that bears more than eight valence electrons.
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how to determine which ion has the lowest charge density?
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the bigger the element, the more spread out it is and it's density is lower (look at radius)
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how to determine lattice energy from given data?
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use the given data to find the energy of the compound with the most similar bond strength, and adjust your expectations of energy according to the electronegativity differences
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what is lattice energy?
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a measure the strength of the bonds in a compound. often referred to as enthalpy of formation.
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what is the electron affinity trend?
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same as electronegativity. highest in top right corner
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what does endothermic electron affinity mean?
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you would have to input energy to make the element accept another electron (it wouldnt easily accept it. endothermic electron affinity would increase as reactivity decreased)
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In general, electrons are removed from the valence-shell __ orbitals before they are removed from valence __orbitals when transition metals are ionized.
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In general, electrons are removed from the valence-shell s orbitals before they are removed from valence d orbitals when transition metals are ionized.
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how to find which is least electronegative?
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follow the electronegativity trend. highest in top right corner, lowest in bottom left corner.
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how to determine bond length?
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single bonds are longest and weakest
double bonds are medium length and medium strength triple bonds are shortest and strongest |
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how to find which bond is most polar?
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look for the biggest differences in electronegativity
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how to find the best choice for ΔH for the reaction?
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draw a bond diagram and find the broken and formed bonds. broken is + energy, formed is - energy.
add broken bond energies and then subtract broken bond energies to find the answer |
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how to find the best choice for fuel value of a compound?
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balance the reaction, then use the process of finding which bonds have been broken and which bonds have been formed. +energy for bonds broken, -energy for bonds formed. to find the fuel value, convert from moles to grams.
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how to find when the ionization potential becomes discontinuous?
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this is when the next electron to be taken (ionized) will come from the core group (no longer from the valence electrons).
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