Download Unit 6 Study Guide – Chemical Bonding 1. A _ chemical

Unit 6 Study Guide – Chemical Bonding
1. A _chemical bond________________ ____________ is a mutual electrical attraction
between the nuclei and valence electrons of different atoms that binds the atoms together.
2. Are atoms more or less stable when they bond? _more stable____________________
3. Chemical bonding that results from the electrical attraction between large numbers of
cations and anions is called __ionic_____________ __bonding__________.
4. __Covalent___________ bonding results from the sharing of electron pairs between two
atoms.
5. How is bonding and potential energy of atoms related? _potential energy decreases when
atoms bond_____________________________________________________________
6. How is the type (ionic or covalent) of bond determined? ____________________
____difference in electronegativity__________________________________________
7. _Electronegativity______________ is a measure of the ability of an atom in a chemical
compound to attract electrons. Which is the most electronegative element? _F___
8. A __nonpolar______________ covalent bond is a covalent bond in which the bonding
electrons are shared equally by the bonded atoms.
9. A _polar_______________ covalent bond is a covalent bond in which the bonded atoms
have an unequal attraction for the shared electrons.
10. Is bonding between two atoms of the same element polar-covalent or nonpolar-covalent?
____nonpolar____________________
11. The greater the electronegativity difference between bonded atoms, the greater
___ionic______________ character the bond has.
12. A _molecule_____________ is a neutral group of atoms held together by covalent bonds.
13. A __chemical_________________ formula indicates the relative numbers of atoms of
each kind in a chemical compound by using atomic symbols and numerical subscripts.
14. A _molecular______________ formula shows the types and numbers of atoms combined
in a single molecule of a molecular (covalent bonding) compound.
15. What is bond length? _see notes_______________________
_______________________________________________________________________
16. What rule or principle states that atoms tend to form compounds so that each atom can
have eight electrons in its outermost energy level? __octet rule_____________________
17. Which group satisfies the octet rule without forming compounds? __noble gases_______
18. Electron-dot notation is used to show the ____________ ____________ of an atom.
19. A __lone pair_________ _________ is a pair of electrons that is not involved in bonding
and that belongs exclusively to one atom.
20. What are Lewis structures? _see notes_______________________________________
________________________________________________________________________
21. Draw the Lewis structure for the following molecular compounds.
3.
4.
5.
6.
NH3
H2S
SiH4
HF
22. An __ionic____________ compound is composed of positive and negative ions that are
combined so that the numbers of positive and negative charges are equal.
23. Most ionic compounds exist as ___crystalline___________ __solids______________.
24. What does a formula unit of an ionic compound indicate? __the number of ions that
balances charge__________________________________________________________
25. _Lattice______________ _energy________________ is the energy released when one
mole of an ionic crystalline compound is formed from gaseous ions.
26. Which has stronger forces of attraction? ionic compounds or molecular compounds
27. A charged group of covalently bonded atoms is known as a _polyatomic____ ion.
28. __Molecular_________________ __geometry___________ is the three-dimensional
arrangement of a molecule’s atoms in space.
29. What is molecular polarity? _uneven distribution of charge in a covalent compound____
30. What theory predicts the shape of molecules based on repulsion between electrons for
each other? __Valence Shell Electron Pair Repulsion (VSEPR)____________________
31. Draw a Lewis structure for each of the following molecules, and then use VSEPR theory
to predict the molecular geometry of each and specify the type of geometry:
a. SCl2 bent
trigonal pyramidal
b. PI3
c. SiCl3Br
tetrahedral
d. NO3
trigonal planar
e. SO42tetrahedral
32. _Hybridization____________________________ is the mixing of two or more atomic
orbitals of similar energies on the same atom to produce orbitals of equal energies.
33. The strength of intermolecular forces is (larger, smaller) than the strength of molecular
bonds.
34. The forces of attraction between polar molecules (those that have positive and negative
regions) are known as __dipole-dipole_______________________ forces.
35. What is hydrogen bonding? _______see notes______________________________
_______________________________________________________________________
36. The intermolecular attraction resulting from the constant motion of electrons and the creation
of instantaneous dipoles are called _London____________ __dispersion_____ forces.
37. A chemical bond formed by the attraction between positive ions and surrounding mobile
electrons is a __metallic______________ bond.
38. What are some characteristics of metals attributed to their bonding? __luster, malleability,
ductility, conductivity_________________
39. Do you expect the PCl3 molecule to be polar or nonpolar? polar
40. Do you expect the BrCl molecule to be polar or nonpolar? polar
41. Do you expect the SnCl4 molecule to be polar or nonpolar? nonpolar
42. A _chemical______________ formula indicates the relative numbers of _atoms___________
of each kind in a chemical formula.
43. For a _molecular______________ compound, the chemical formula reveals the number of
atoms of each element contained in a single molecule of the compound.
44. The chemical formula for a _ionic_____________ compound represents one formula unit –
the simplest ratio of the compound’s positive and negative ions.
45. The explosive TNT has the molecular formula C7H5(NO2)3. How many elements make up
this compound? __4____________ How many oxygen atoms are present in one molecule of
this compound? __6_____________ How many atoms in total are present in one molecule
of this compound? __21_______________.
46. Which type of elements tend to form covalent bonds? __nonmetals___________________
47. Which type of elements tend to form ionic bonds? _____metals and nonmetals__________