Chemistry Unit 5
Unit 5: Chemical Bonding, Structure, and Nomenclature
Part A Study Guide
1. Be able to define:
• Anion – an ion with a negative charge because it has more electrons than protons
• Bond angle – the angle that forms between two bonds to a single atom
• Bond length – the distance between the nuclei of two atoms that are bonded to each other
• Cation – an ion with a positive charge because it has more protons than electrons
• Chemical bond – the forces that hold atoms or ions together in a compound
• Chemical structure – the way the compound’s atoms are bonded to make the compound
• Compound – made of two or more elements that are chemically combined
• Covalent bond – atoms that are joined by sharing electrons
• Diatomic molecule – a molecule consisting of two atoms, typically they are the same
element
• Double bond – two pairs of electrons are shared by two atoms
• Intermolecular forces – forces that exist between molecules.
o Ex: ion-dipole interactions, dispersion forces, dipole interactions, hydrogen
bonding
• Intramolecular forces – forces that hold one atom to another to form a new substance
o Ex: ionic bonding, covalent bonding, metallic bonding
• Ion – an atom with an imbalance in protons and electrons
• Ionic bond – a bond that forms when electrons are transferred between two atoms
• Lone pair – pairs of electrons that only belong to one atom and are not shared
• Molecule – a group of atoms held together by covalent bonds
• Network solid – solids with a very orderly pattern that tends to have very high melting
points and boiling points
• Octet Rule – states the atoms want to achieve the electron configuration of a Noble Gas
(they want eight valence electrons)
• Single bond – one pair of electrons is shared by two atoms
• Space-filling model – models that show the space the atoms take up or fill when in a
compound
• Structural formula – it shows the structure of a compound
• Triple bond – three pairs of electrons are shared by two atoms
• Valence electron – the electrons in the highest occupied energy level of an atom
2. Which subatomic particle determines the properties of an element? electron
3. How many valence electrons are transferred from the oxygen atom to the sodium in the formation of
the compound sodium oxide? Oxygen transfers no electrons to one sodium atom.
4. Ionic compound are made of _______________ and _______________. Cations and anions,
metals and nonmetals
5. What is the name of an ionic compound formed from aluminum and sulfur? aluminum sulfide
6. List the prefixes and the numbers that correspond to each prefix.
• 1 = mono-
• 2 = di-
• 3 = tri-
• 4 = tetra-
• 5 = penta-
• 6 = hexa-
• 7 = hepta –
• 8 = octa-
• 9 = nona-
• 10 = deca-
7. Name a diatomic molecule with a triple bond. N2
8. How many electrons are transferred from the potassium atom to the nitrogen atom in the formation
of potassium nitride? Potassium gives one electron to nitrogen. Two more potassium ions are
required in order to get all the electrons that nitrogen would need.
9. The net charge of an ionic compound is _______________. zero
10. Name a pair of atoms that would form a covalent bond. Any nonmetal another nonmetal. You can
occasionally have a metalloid with a nonmetal.
11. What are the diatomic molecules? H2, N2, O2, F2, Cl2, Br2, I2
12. How does nitrogen obey the octet rule when forming compounds? Nitrogen gains three electrons.
13. How can we show chemical structure? We can use one of several models to show how the atoms are
connected to each other.
14. Name a diatomic molecule with a single bond. H2, F2, Cl2, Br2, I2
15. Molecular compounds are formed from two _______________. nonmetals
16. The __________ states that atoms tend to have the electron configuration of a noble gas in
chemical compounds. Octet rule
17. What is the name of an ionic compound between lithium and chlorine? Lithium chloride
18. What kinds of ions have an ending of –ide? nonmetals
19. Why are bond angles and bond lengths averages? Atoms are constantly moving so that changes bond
lengths and bond angles slightly.
20. Oppositely charged ions are attracted in ______________. Ionic bonds
21. What is the name of an ionic compound formed from strontium and bromine? Strontium bromide
22. What does it mean to not obey the octet rule? What would be an example of that? Not obeying the
octet rule would mean to have more or less electrons than eight valence electrons.
23. Name a diatomic molecule with a double bond. O2
24. Name a pair of atoms that would form a covalent compound. Any nonmetal another nonmetal. You
can occasionally have a metalloid with a nonmetal.
25. Cations are found among __________ on the Periodic Table, and anions tend to be found among
__________. Metals, nonmetals
26. Name a pair of atoms that would form an ionic bond. Any metal with a nonmetal, a metal with a
polyatomic ion, or any two polyatomic ions.
27. How does calcium obey the octet rule when forming compounds? Calcium loses 2 electrons
28. How do chemical bonds form? Chemical bonds form when electrons are transferred or shared in
order to create a force to hold atoms together.
29. Why are different models of molecular structure valuable? Different models show us different types
of information about the structure and size of a molecule.
30. How does oxygen obey the octet rule when forming compounds? It gains 2 electrons.
31. Name a pair of atoms that would form an ionic bond. Any metal with a nonmetal, a metal with a
polyatomic ion, or any two polyatomic ions.
32. Why is the structure of a substance important? Structure is important because it can dictate the
properties that the substance will have.
33. Why do we use Roman numerals when writing the name for ionic compounds that use transition
metals? Transition metals can have multiple charges, so we need to use Roman numerals to
identify which charge exists in that compound. This helps prevent confusion and ensures that the chemical formula accurately reflects the composition and oxidation state of the metal involved.