04:47Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius, and Electron AffinityLondon Jenks593views
07:53The Periodic Table: Atomic Radius, Ionization Energy, and ElectronegativityProfessor Dave Explains723views
Multiple ChoiceArrange the following atoms and/or ions in the order of increasing size:Br –, Kr, Rb+, Sr2+.1798views7rank
Multiple ChoiceFor an isoelectronic series of ions, the ion that is the smallest is always 1860views6rank
Textbook QuestionConsider the Mg2+, Cl-, K+, and Se2- ions. The four spheres below represent these four ions, scaled according to ionic size. (b) In terms of size, between which of the spheres would you find the (i) Ca2 + and (ii) S2 - ions? 965views
Textbook QuestionWhich of the following spheres is likely to represent a metal atom and which a nonmetal atom? Which sphere in the products represents a cation and which an anion? 966views
Textbook QuestionConsider the ionic compounds KF, NaCl, NaBr, and LiCl. (a) Use ionic radii (Figure 7.8) to estimate the cation–anion distance for each compound.1041views
Textbook QuestionIdentify each statement as true or false: (a) Cations are larger than their corresponding neutral atoms.521views
Textbook QuestionConsider S, Cl, and K and their most common ions.(c) Explain any differences in the orders of the atomic and ionic sizes.649views
Textbook QuestionArrange each of the following sets of atoms and ions, in order of increasing size: (a) Pb, Pb2+, Pb4+1030views
Textbook QuestionProvide a brief explanation for each of the following.K+ is larger than Na+.934views
Textbook QuestionIn the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 201 pm (Li–F), 282 pm (Na–Cl), 330 pm (K–Br), and 367 pm (Rb–I), respectively. (b) Calculate the difference between the experimentally measured ion–ion distances and the ones predicted from Figure 7.8. 857views
Textbook QuestionIn the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 201 pm (Li–F), 282 pm (Na–Cl), 330 pm (K–Br), and 367 pm (Rb–I), respectively. (c) What estimates of the cation– anion distance would you obtain for these four compounds using neutral atom bonding atomic radii? Are these estimates as accurate as the estimates using ionic radii?1321views
Textbook QuestionWhich atom or ion in the following pairs would you expect to be larger? (c) O-or O2-726views
Textbook QuestionWhich atom or ion in the following pairs would you expect to be larger? (c) Cr3+ or Cr6+547views
Textbook QuestionThe following ions all have the same number of electrons: Ti4+, Sc3+, Ca2+, S2-. Order them according to their expected sizes, and explain your answer.1119views
Textbook QuestionWhich is the larger species in each pair? a. Li o r Li+ b. Cs- o r Cs+ c. Cr- or Cr3+ d. O or O2-3376views1rank
Textbook QuestionWhich is the larger species in each pair? a. Sr or Sr2+ b. N or N3- c. Ni or Ni2+ d. S2-or Ca2+1642views
Textbook QuestionArrange this isoelectronic series in order of increasing atomic radius: Se2 - , Sr2 + , Rb+ , Br - .5123views1rank2comments
Open QuestionThe following ions contain the same number of electrons. rank them in order of decreasing ionic radii.272views
Open QuestionCations have a ______________ charge and are ______________ than the atoms from which they formed.124views
Open QuestionWhich of the following ranks these isoelectronic species in order of increasing atomic radii?138views
Multiple ChoiceArrange the following isoelectronic series in order of decreasing radius: F–, O2– , Mg2+, Na+.15views