04:47Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius, and Electron AffinityLondon Jenks606views
07:53The Periodic Table: Atomic Radius, Ionization Energy, and ElectronegativityProfessor Dave Explains737views
Multiple ChoiceArrange the following atoms and/or ions in the order of increasing size:Br –, Kr, Rb+, Sr2+.1814views7rank
Multiple ChoiceFor an isoelectronic series of ions, the ion that is the smallest is always 1883views6rank
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? 995views
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? 978views
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.1055views
Textbook QuestionIdentify each statement as true or false: (a) Cations are larger than their corresponding neutral atoms.525views
Textbook QuestionConsider S, Cl, and K and their most common ions.(c) Explain any differences in the orders of the atomic and ionic sizes.656views
Textbook QuestionArrange each of the following sets of atoms and ions, in order of increasing size: (a) Pb, Pb2+, Pb4+1040views
Textbook QuestionProvide a brief explanation for each of the following.K+ is larger than Na+.944views
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. 870views
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?1332views
Textbook QuestionWhich atom or ion in the following pairs would you expect to be larger? (c) O-or O2-735views
Textbook QuestionWhich atom or ion in the following pairs would you expect to be larger? (c) Cr3+ or Cr6+553views
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.1133views
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 O2-3396views1rank
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+1661views
Textbook QuestionArrange this isoelectronic series in order of increasing atomic radius: Se2 - , Sr2 + , Rb+ , Br - .5163views1rank2comments
Open QuestionThe following ions contain the same number of electrons. rank them in order of decreasing ionic radii.283views
Open QuestionCations have a ______________ charge and are ______________ than the atoms from which they formed.129views
Open QuestionWhich of the following ranks these isoelectronic species in order of increasing atomic radii?142views
Multiple ChoiceArrange the following isoelectronic series in order of decreasing radius: F–, O2– , Mg2+, Na+.16views