(a)
Interpretation:
From the given pair elements the one with more non-metallic character has to be predicted.
Concept introduction:
Periodic properties
The metallic character decreases in a period from left to right in the periodic table.
The metallic character increase in a group from top to bottom.
(b)
Interpretation:
From the given pair of elements the one with more non-metallic character has to be predicted.
Concept introduction:
Metallic property
The metallic character decreases in a period from left to right in the periodic table.
The metallic character increase in a group from top to bottom.
(c)
Interpretation:
From the given pair elements the one with more non-metallic character has to be predicted.
Concept introduction:
Metallic property
The metallic character decreases in a period from left to right in the periodic table.
The metallic character increase in a group from top to bottom.
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General Chemistry: Atoms First
- Write the electron configurations for the following atoms or ions:(a) B3+(b) O–(c) Cl3+(d) Ca2+(e) Tiarrow_forwardPredict the best choice in each of the following. You may wish to review the chapter on electronic structure for relevant examples.(a) the most metallic of the elements Al, Be, and Ba(b) the most covalent of the compounds NaCl, CaCl2, and BeCl2(c) the lowest first ionization energy among the elements Rb, K, and Li(d) the smallest among Al, Al+, and Al3+(e) the largest among Cs+, Ba2+, and Xearrow_forwardWrite the electron configurations for the following atoms or ions: (a) B3+ (b) O– (c) Cl3+ (d) Ca2+ (e) Tiarrow_forward
- (a) (i) (ii) (iii) With the aid of a simple schematic, explain what covalent bonding is and how it is formed. What are the differences between a covalent bond and an ionic bond? Which type of bond is found in crystalline silicon? At room temperature do you expect an ionic crystal to be a good electrical conductor or a good electrical insulator? Explain why.arrow_forward8a) Sketch a diagram showing the formation of energy levels from the valence orbitals for Rb, Rb2, Rb3, and Rbn. On the diagram, place arrows indicating how the electrons fill these energy levels. b) How many energy levels are present in the valence band of a single crystal of rubidium with a mass of 48.3 g?arrow_forward(a) What are the common oxidation states of the halogens?(b) Give an explanation based on electron configuration for the range and values of the oxidation states of chlorine.(c) Why is fluorine an exception to the pattern of oxidation states found for the other group members?arrow_forward
- Element X is a metal with a valency 2. Element Y is a non-metal with a valency 3 (a) Write equations to show how X and Y form ions. (b) If Y is a diatomic gas, write the equation for the direct combination of X and Y to form a compound.arrow_forwardConsider these statements about an element E in Group 4A: • The most important modern use of E is as an ultrapure semiconductor used to make microelectronic chips. • E has two main allotropes: a shiny silvery-white metal at room temperature, and a brittle gray powdery form at colder temperatures. • Although E is not a common element on the Earth's crust, deposits of the mineral EO₂ are widely found, and this ore can be reduced to E with moderate heating and charcoal. • Under standard conditions, E is a metal. Are all of these statements true about the same Group 4A element? If you said yes, what is E? Enter its chemical symbol: O O 0 yes no X Sarrow_forward(a) The third row element with the largest first ionization energy. (b) The Group 3A element with the largest first ionization energy. (c) The Group 3A element with the largest atomic radius.arrow_forward
- The elements sodium, aluminum, and chlorine are in the same period. (a) Which has the greatest electronegativity? (b) Which of the atoms is smallest? (c) Which is the largest possible oxidation state for each of these elements? (d) Will the oxide of each element in the highest oxidation state (write its formula) be acidic, basic, or amphoteric?arrow_forward24. Which member of the following pairs has the larger radius? Provide your reasoning. (a) Al or S (b) Cl or Ca²+ (c) Ba or Sn (d) Na+ or Karrow_forwardEnergy 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.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax