(a)
Interpretation:
The type of bond present in a compound formed from magnesium and chlorine is to be predicted.
Concept introduction:
Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are the result of the electronegativity difference between bonding atoms. If the electronegativity difference is
(b)
Interpretation:
The type of bond present in a compound formed from carbon and hydrogen is to be predicted.
Concept introduction:
Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are the result of the electronegativity difference between bonding atoms. If the electronegativity difference is
(c)
Interpretation:
The type of bond present in a compound formed from phosphorus and hydrogen is to be predicted.
Concept introduction:
Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are the result of the electronegativity difference between bonding atoms. If the electronegativity difference is
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Chemistry for Today: General, Organic, and Biochemistry
- In forming an ionic bond with an atom of chlorine, a sodium atom will: a.receive one electron from the chlorine atom. b.receive two electrons from the chlorine atom. c.give up one electron to the chlorine atom. d.give up two electrons to the chlorine atom.arrow_forwardWhich type of bond is most common between metal and nonmetal elements? A. Ionic B. Covalent C. Hydrogen D. Refractoryarrow_forward1. How many electrons will an iodine atom donate or accept, based on its number of valence electrons? A. Donate 7 electrons B. Donate 1 electron C. Accept 7 electrons D. Accept 1 electrons 2.What type of bond is formed between the two nitrogen atoms in diatomic nitrogen, N2? A. Triple Bond B. Double Covalent Bond C. Double Ionic Bond D. Single Bond 3.Which metal would form a stronger metallic bond? A. Lithium B. Sodium C. Strontium D. Tungsten 4. What holds the metal ions together in a lattice? A. Hydrogen Bonds B. Covalent Bonds C. Metallic Bonds D. Ionic Bondsarrow_forward
- Which type of bond results from the sharing of electron(s) between two atoms? A. Ionic B. Covalent C. Hydrogen D. Electrovalentarrow_forwardTTT One or more positively-charged 1 negatively-charged atoms. A. Ionic bond B. Covalent bond atoms are electrostatically bound to one or more C. Metallic bond D. Hydrogen bond Hydrogen atoms are attached to a very electronegative atom. The hydrogen atom on 2 one molecule is attracted to the electronegative atom on another molecule. A. Ionic bond C. Metallic bond B. Covalent bond D. Hydrogen bond Electrons are not shared. Atoms have gained or lost valence electrons such that they 3 have a full octet of valence electrons. A. Ionic bond B. Covalent bond A. Ionic bond B. Covalent bond C. Metallic bond D. Hydrogen bond Atoms share two or more valence electrons with other atoms such that they have a 4 full octet of valence electrons. C. Metallic bond D. Hydrogen bond 5 The strongest type of chemical bond. A. Ionic bond B. Covalent bond C. Metallic bond D. Hydrogen bond Atoms are so tightly packed together that their valence electrons move freely from 6 atom to atom. A. Ionic bond B.…arrow_forwardChapter 4 Worksheet Answer the following questions. Be sure to check your spelling. In ionic compounds, positively charged a. metals, anions b. nonmetals, cations c. metals, polyatomic ions d. nonmetals, anions e. metals, cations A) lose their valence electrons to become An ionic compound a. has a net positive charge. b. has a net negative charge. c. contains only cations. d. contains only anions. e. has a net charge of zero. 3) Which of the following compounds contains an ionic bond? a. NH3 b. H2О с. СаО d. H2 A group of covalently bonded atoms that has an overall electrical charge is called a(n) a. ionic compound. b. anion c. polyatomic ion. d. cation. e. molecule. In a molecule with covalent bonding, a. oppositely charged ions are held together by strong electrical attractions. b. atoms of metals form bonds to atoms of nonmetals. c. atoms of different metals form bonds. d. atoms are held together by sharing electrons. 10arrow_forward
- Which pairs of elements will form ionic compounds? a. lithium and bromine c. calcium and magnesium b. chlorine and oxygen d. barium and chlorinearrow_forwardIn a covalent bond A. Two ions come together and form a crystal lattice. B. Two elements react in forming new compound C. Two Atoms exchange electrons in the atoms are attracted to each other. D. Two Atoms share valence electrons in those shared electrons form the chemical bond.arrow_forwardLabel the bond formed between carbon and each of the following elements as nonpolar, polar, or ionic. a. carbon b. oxygen c. lithium d. chlorine e. hydrogenarrow_forward
- Which type of bond is most likely to form between two atoms of Carbon? A. Ionic B. Polar Covalent C. Nonpolar Covalent D. Hydrogenarrow_forward1. Compare the lattice energies of Cao and Mg0 by: a. Writing out the reaction equation associated with the lattice energy for MgO. b. Using Coulomb's Law to clearly and completely explain the difference between MgO and Cao lattice energies in terms of specific scientific principles as discussed in lecture. 2. Write the correct formula for the following ionic compounds: a. Aluminum Acetate b. Ammonium Sulfate C. Calcium Phosphate 3. Draw the complete Lewis structures for each of the following; be sure to include all nonzero formal charges and resonance structures if applicable. a. SCN lon (hint add one additional valence electron for-1 lons) b. Co: ion (hint: add two additional valence electrons for -2 ions) C OF d. PH3 e. CH;CH; f. N;Haarrow_forward1. Use your knowledge of the element groups in the periodic table to determine the formula for a compound containing potassium (K) and bromine (Br). 2. Determine the formula for a compound containing cesium (Cs) and sulfur (S). 3. Write an equation for the formation of the following compounds from their ions: a. BeSe b. Na P c. Potassium sulfide d. Calcium chloride -Salts are lonic Compounds 1. Why are ions formed by gaining or losing electrons? What would happen to an atom if a proton were removed? 2. How does electron transfer explain salt formation? BR₂ Focusarrow_forward
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