13% 8:08 PM docs.google.com Covalent Bonding and lonic Bonding study guide T-Mob
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13% 8:08 PM docs.google.com Covalent Bonding and lonic Bonding study guide T-Mobile LTE Note compare and contrast does not mean state one similarity and one difference Go back to our thinking maps and metacognitive logs and review everything we learned. Differentiate between the following: Atom, element, compound, bond, electron. Click here for a short video 2 Compare and contrast ionic and covalent bonds including the nature of the bonds. Click here for a video comparing the 2. Click here for a video on covalent bonding. s Explain the rules used for naming ionic compounds as well as those used for naming molecular compounds. You can either create 2 lists or 1 double bubble. 4 Use the periodic table to indicate whether the following molecules are ionic or covalent. Work each problem using either the diagram for transfer or sharing, then write the chemical formula and finally name each compound correctly. a NaBr b. HF d H20 s Explain why all of the following compounds will be molecular, then draw structural formulas for the following each. a PCI3 b CBr4 NH3 N2 e How many bonds can each of the following atoms form? Explain how you were able to determine the number a Nitrogern b. sulfur Oxygen d fluorine A halogen Carbon For naming molecular compounds apply the following rules: Name the first element in the molecular formula first using the element name without adding a suffix Name the 2nd element using the root of its name only and adding the suffix -ide . Use Greek prefixes (mono 1, di 2, tri 3, tetra 4, penta 5. hexa 6, octa, 8, nona 9, deca 10) to indicate the number of atoms within that binary molecule. For Note: mono is not used as a prefix for the name of the first element. example, for CO2 we day carbon dioxide, not monocarbon dioxide 7. First, determine whether each of the following is an ionic or molecular compound. Then, apply the rules above, or the rules for ionic compounds, and name each of the following binary compounds: a P4010 bAl203 N203 d. SiF6Explanation / Answer
1.
An atom is the smallest entity of a matter that has the properties of an element.
A chemical element is a species of atoms having the same number of protons (atomic no.) in their atomic nuclei.
A chemical compound is formed from atoms of different chemical elements. The different atoms are joined by chemical bonds.
A chemical bond is a combination between atoms, ions or molecules that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between oppositely charged ions (ionic bonds) or through the sharing of electrons (covalent bonds).
The electron is a subatomic particle, symbol e or , whose electric charge is negative one elementary charge.
2.
Ionic bonding is a type of chemical bond that involves the electrostatic attraction between oppositely charged ions. The ions are atoms that have gained one or more electrons and are negatively charged (known as anions) and atoms that have lost one or more electrons and are positively charged (known as cations). E.g. NaCl
A covalent bond, is a chemical bond that involves the sharing of electron pairs between atoms. These electron pairs form -bonds and/or -bonds when they share electrons to attain the equivalent of a full outer shell, corresponding to a stable electronic configuration. E.g. O2
4.
a) [Na+] [Br-] : Sodium Bromide – Ionic Bonding by transfer of 1 electron
b) H-F : Hydrogen Fluoride – Covalent Bonding by sharing of 1 electron each, single bond
c) [Ca2+] [S2-] : Calcium Sulphide – Ionic Bonding by transfer of 2 electrons
d) H-O-H : Water - Covalent Bonding by sharing of 1 electron each, 2 single bonds
e) [Li+] [I-] : Lithium Iodide – Ionic Bonding by transfer of 1 electron
f) N N: Nitrogen - Covalent Bonding by sharing of 3 electrons each, triple bond
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