04:47Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius, and Electron AffinityLondon Jenks616views
07:53The Periodic Table: Atomic Radius, Ionization Energy, and ElectronegativityProfessor Dave Explains744views
Multiple ChoiceArrange the following atoms and/or ions in the order of increasing size:Br –, Kr, Rb+, Sr2+.1821views7rank
Multiple ChoiceFor an isoelectronic series of ions, the ion that is the smallest is always 1894views6rank
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? 1006views
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? 986views
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.1061views
Textbook QuestionIdentify each statement as true or false: (a) Cations are larger than their corresponding neutral atoms.531views
Textbook QuestionConsider S, Cl, and K and their most common ions.(c) Explain any differences in the orders of the atomic and ionic sizes.659views
Textbook QuestionArrange each of the following sets of atoms and ions, in order of increasing size: (a) Pb, Pb2+, Pb4+1046views
Textbook QuestionProvide a brief explanation for each of the following.K+ is larger than Na+.949views
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. 879views
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?1339views
Textbook QuestionWhich atom or ion in the following pairs would you expect to be larger? (c) O-or O2-742views
Textbook QuestionWhich atom or ion in the following pairs would you expect to be larger? (c) Cr3+ or Cr6+556views
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.1140views
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 O2-3405views1rank
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+1675views
Textbook QuestionArrange this isoelectronic series in order of increasing atomic radius: Se2 - , Sr2 + , Rb+ , Br - .5185views1rank2comments
Open QuestionThe following ions contain the same number of electrons. rank them in order of decreasing ionic radii.287views
Open QuestionCations have a ______________ charge and are ______________ than the atoms from which they formed.133views
Open QuestionWhich of the following ranks these isoelectronic species in order of increasing atomic radii?144views
Multiple ChoiceArrange the following isoelectronic series in order of decreasing radius: F–, O2– , Mg2+, Na+.18views