Question

Ionic & Covalent Virtual Lab Pre-Virtual Lab Questions: Answer these before going to the website to begin the virtual lab. 1. Where are metal atoms located on the periodic table? Where are non metal atoms located on the periodic table? 2. What subatomic particles) participate in chemical bonding? 3. In your own words, define valence electrons. 4. How can you determine the number of valence electrons in an atom using the periodic table? 5. Draw a Lewis Dot Structure for the following atoms a. Strontium (SI) b.Carbon ( c. Iodine (0) d. Xenone) Part I: Ionic Bonding 1. Choose Sodium (Na). a. What type of element is it? b. How many valence electrons does it have? 2. Choose Fluorine (F). a. What type of element is it? b. How many valence electrons does it have? 3. Answer the question on the screen, "What type of bond is this combination likely to form?" a Circle: Ionic or Covalent? b. Choose the appropriate number of atoms to make the bond. Record the number of each atom below: 4. Watch the final animation closely it will play continuously). a. Describe the change in the number of valence electrons in the atoms as the bond is successfully formed b. What does the positive (+) charge indicate (mention specific subatomic particles in your answer?

Answer 1

Pre-virtual lab questions:
1. Metal atoms lie on the left side of the periodic table and non-metals lie on the right side.
Group 1: Alkali metals
Group 2: Alkaline earth metals
Group (3 to 12): Transition elements (all metals)
Non-metals(except hydrogen) belong to the p-block of the periodic table.

2. Electrons are the sub-atomic elements that participate in the chemical reactions. Elements react either by transfer of electrons or by sharing of electrons.

3. Valence electrons are the electrons present in the valence shell of the atom.

4. The elements belonging to the same group in the periodic table have the same number of valence electrons.
Group 1: 1 valence electron
Group 2: 2 valence electrons
Group 13: 3 valence electrons
Group 14: 4 valence electrons
Group 15: 5 valence electrons
Group 16: 6 valence electrons
Group 17: 7 valence electrons
Group 18: 8 valence electrons

5.

Part I: Ionic Bonding
1. a. Na(Sodium) is a metal.
b. It has 1valence electron.

2. a. (F) Fluorine is a non-metal.
b. It has 7 valence electrons.

2. a. Oxygen atom has 6 valence electrons.
b. It is a non-metal.
c. Two Oxygen atoms combine by sharing two pairs of electrons between them.
A bond formed by sharing is a covalent bond.
d.  A covalent bond is formed by overlapping of atomic orbitals to create a molecular orbital.
e. Two Fluorine atoms combine by a single covalent bond by sharing one pair of electrons between them.
Two oxygen atoms combine by a double covalent bond by sharing two pairs of electrons between them.

Part III: Critical thinking
1. Atoms participate in chemical bonding in order to acquire a stable octet configuration.
An ionic bond is formed by transfer of electrons between metals and non-metals. The metalic elements have less than 4 valence electrons and lose electrons to form cations. The non-metalic elements have 4 or more valence electrons and gain electrons to form anions. In an ionic bond these ions are held together by electrostatic forces of attraction.
A covalent bond is formed by sharing of electrons between atoms of valence electrons.

3. Note: bonds between metals and non-metals may be covalent due to polarization of the electron cloud of the anion by the cation.

a. Sr. (Strontium) b. .C. (Carbon) c. :i: (lodine) d. : Xe : (Xenon)

Name	Formula	Ionic or covalent
Beryllium Bromide	BeBr2	Covalent
Phosphorus trifluoride	PF3	Covalent
Sulphur diodide	SI2	Covalent
Strontium phosphide	Sr3P2	Ionic bond with a covalent character
Cesium nitride	Cs3N	Ionic
Water	H2O	Polar covalent bond

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