What correlation, if any, exists for the Period 2 elements be-tween group number and the number of covalent bonds the ele-ment typically forms? How is the correlation different for elements in Periods 3 to 6?

.9% Resources O Hint Consider an ionic compound, MX,, composed of generic metal M and generic gaseous halogen X. • The enthalpy of formation of MX, is AH; = -605 kJ/mol. • The enthalpy of sublimation of M is AHsub = 129 kJ/mol. • The first, second, and third ionization energies of M are IE, = 691 kJ/mol, IE2 = 1581 kJ/mol, and IE3 = 2627 kJ/mol. • The electron affinity of X is AHEA = -361 kJ/mol. (Refer to the hint). • The bond energy of X, is BE = 163 kJ/mol. Determine the lattice energy of MX3. AHjattice kJ/mol about us privacy policy terms of use contact us help careers

Energy is required to remove two electrons from Ca to formCa2+, and energy is required to add two electrons to O toform O2 - . Yet CaO is stable relative to the free elements.Which statement is the best explanation? (a) The latticeenergy of CaO is large enough to overcome these processes.(b) CaO is a covalent compound, and these processes areirrelevant. (c) CaO has a higher molar mass than either Ca orO. (d) The enthalpy of formation of CaO is small. (e) CaO isstable to atmospheric conditions.

The electron configurations for four main-group elements are given. Match the electron configuration on the left with the Lewis structure on the right. Clear All 1s²2s-2p°3s°3p°4s°3a104p°5s' 1s²2s-2p°3s²3p°4s°3a'04p² X• 1s 25 2p5 :*: 1s2s-2p°3s²3p° :*:

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BOTH PLEASE Consider an ionic compound, MX,, composed of generic metal M and generic gaseous halogen X. • The enthalpy of formation of MX, is AH; = -739 kJ/mol. • The enthalpy of sublimation of M is AHub = 131 kJ/mol. • The first, second, and third ionization energies of M are IE, = 635 k/mol, IE, = 1575 kl/mol, and IE, = 2629 kJ/mol. • The electron affinity of X is AHEA = -327 kJ/mol. (Refer to the hint). • The bond energy of X, is BE = 229 kJ/mol. Determine the lattice energy of MX,. ΔΗ kJ/mol TOOLS x10 Consider the following information. • The enthalpy of formation of BaO is AH; = -548.0 kJ/mol. • The enthalpy of sublimation of Ba is AH ub = 180.0 kJ/mol. • The first and second ionization energies of Ba are IE, = 503 kJ/mol and IE, = 965 kJ/mol. • The first electron affinity of O is AHEAI = -142 kJ/mol. • The bond energy of O, is BE = 498 kJ/mol. • The lattice energy of BaO is AHice = -3029 kJ/mol. Determine the second electron affinity of O. AHEAZ= kl/mol

List the order in which the orbitals are filled as the atoms beyond hydrogen are built up. How many electrons overall can be accommodated in the first and second principal energy levels? How many electrons can be placed in a given s subshell? In a given p subshell? In a specific p orbital? Why do we assign unpaired electrons in the 2p orbitals of carbon, nitrogen, and oxygen?

For each of the following atoms or ions, state the total number of electrons, the number of valence electrons, and the number of core electrons. (a) Rn (b) Sr+ (c) Se2 (d) Sb2

Before the element scandium was discovered in 1879, it was known as “eka-boron.” Predict the properties of scandium from averages of the corresponding properties of its neighboring elements in the periodic table. Compare your predictions with the observed values in Appendix F.

Why do most monatomic cations of the main-group elements have a charge equal to the group number? Why do most monatomic anions of these elements have a charge equal to the group number minus eight?