O (oxygen) Enter the full electron configuration for Cl−. Neon What element forms an ion with an electronic configuration of 1s22s22p6 (or ) and a −2 charge? Give the symbol for the element. Which noble gas electron configuration is attained in this process? 2 electons How many electrons must be lost by the element Mg? Ne Metals lose electrons under certain conditions to attain a noble gas electron configuration. Most Energy released by gaining an electron to most energy absorbed by gaining an electron. between the first and second ionization energies Predict where the largest jump between successive ionization energies occurs for Mg Between the second and third ionization energies The elements of which group in the periodic table release the most energy by gaining an electron? 7A The elements of which group in the periodic table absorb the most energy when gaining an electron? 8A Arrange these elements according to electron affinity. Rb Predict where the largest jump between successive ionization energies occurs for K.
Na Arrange these elements according to first ionization energy. K+ Arrange these ions according to ionic radius.Ĭa2+ Arrange these elements according to first ionization energy. Oxygen Arrange the atom and ions according to radius. Ne Arrange the elements according to atomic radius, from largest to smallest. Largest to SmallestĬ Arrange these elements according to atomic radius. Rb Arrange these elements according to atomic radius. Kr: Rb+ Rank the elements by effective nuclear charge, 𝑍eff, for a valence electron. +7 Match each of the ions with the noble gas that has the same number of electrons. Kr: 8 Identify the number of core and valence electrons for Ar 10 core electrons andĨ valence electrons Identify the number of core and valence electrons for Ca: 18 core and 2 valence electrons Identify the number of core and valence electrons for I 46 core electrons and 7 valence electrons The effective nuclear charge, 𝑍effZeff, for a valence electron can be approximated using the core charge of the atom that is, the net charge of the nucleus and the inner (nonvalence) electrons.ĭetermine the core charge for an atom of Cl. For example, if an atom has two valence electrons, enter the number 2. N: 5 Determine the number of valence electrons for each of the atoms. Si 4 Determine the number of valence electrons for each of the atoms. For example, if an atom has two valence electrons, enter the number 2.Ĭ: 4 Determine the number of valence electrons for each of the atoms. N=7, l=1, ml=-1 2 Determine the number of valence electrons for each of the atoms. N=4, l=1 6 How many electrons in an atom could have these sets of quantum numbers? N=3 18 How many electrons in an atom could have these sets of quantum numbers?
(ml) = -4 g How many electrons in an atom could have these sets of quantum numbers? (ml) = -1 g, f, d, p Which subshells (𝑠, 𝑝, 𝑑, 𝑓, or 𝑔)(s, p, d, f, or g) can have electrons with the indicated magnetic quantum number (𝑚𝓁)? (ml) = 3 g, f Which subshells (𝑠, 𝑝, 𝑑, 𝑓, or 𝑔)(s, p, d, f, or g) can have electrons with the indicated magnetic quantum number (𝑚𝓁)? (ml) = 0 d, f, p, g, s Which subshells (𝑠, 𝑝, 𝑑, 𝑓, or 𝑔)(s, p, d, f, or g) can have electrons with the indicated magnetic quantum number (𝑚𝓁)? Identify all allowable combinations of quantum numbers for an electron.
The four quantum numbers, the principal quantum number (𝑛), the angular momentum quantum number (𝓁), the magnetic quantum number (𝑚𝓁), and the spin quantum number (𝑚s) have strict rules which govern the possible values. What quantum numbers specify 5s n=5 and l=0 What quantum numbers specify 6p n=6 and l=1 Quantum numbers arise naturally from the mathematics used to describe the possible states of an electron in an atom.
0 kommentar(er)
