Questions and Answers
When sharing of electrons occurs, the attachment between atoms is called?
covalent bond
In a covalent bond, the dissociation energy is released in the process of?
exothermic reaction
When 2 or more atoms bond by means of electron sharing, the result is?
a molecule
Shared electrons are centered between the 2 atoms in covalent bonding, the attachment is called?
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In covalent bonding, where there is an overlap of parallel orbitals, this type of attachment occurs?
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In what form do electrons such as hydrogen, nitrogen, and oxygen normally occur?
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How many electrons are shared in a double covalent bond?
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Bond length is the distance between?
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Which form of relationships relating to bond length is normally correct?
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Binary molecular compounds are generally composed of a metal and a nonmetal.
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The 2nd element in the formula of a binary compound is named using the suffix -ite.
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The prefix 'tetra-' means 3 atoms.
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The prefix 'hexa-' means 6 atoms.
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When naming the 1st element in a formula, the prefix 'mono-' is not used.
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For binary acids, the hydrogen part of the compound is named using the prefix 'hydro-'.
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An oxyacid contains 2 elements.
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If the name of the anion of an oxyacid ends in '-ate', the acid name ends in '-ous'.
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What is CO?
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What is CO2?
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What is H2CO3?
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What is NH3?
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What is N2O4?
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What is HNO2?
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What is HNO3?
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What is HBr?
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What is HBrO3?
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A structural formula shows the arrangement of the atoms in a molecule.
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The central atom in a molecule is the one with the higher electron affinity.
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In molecules, hydrogen is always a terminal atom.
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The number of bonding pairs in a molecule is equal to the number of electrons.
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To find the total number of electrons available for bonding in a + ion, you should add the ion charge to the total number of valence electrons of the atoms present.
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The electrons in a coordinate covalent bond are donated by both the bonded atoms.
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Resonance occurs when more than 1 valid Lewis structure can be written for a molecule.
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Nitrate is an example of an ion that forms resonance structures.
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The carbon dioxide molecule contains 2 double bonds.
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All electrons in an atom are available for bonding.
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In the sulfate ion (SO4^2-), 32 electrons are available for bonding.
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When carbon and oxygen bond, the molecule contains 10 pairs of bonding electrons.
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What is O3?
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What is BF3?
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What is NO?
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What is SF6?
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What determines molecular shape?
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Bond angle is an angle between?
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VSEPR model is based on what idea?
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What is a tetrahedral molecule?
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What is a linear molecule?
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What is a trigonal pyramidal molecule?
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What is hybridization?
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In hybridization?
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What is sp3?
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What is electronegativity?
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What is the element with the highest electronegativity and its numerical value?
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Name and group number of the family with the highest overall electronegativities.
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What is the element with the lowest electronegativity and its numerical value?
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Name and group number of the chemical family that has the lowest overall electronegativities.
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Ionic compounds are usually soluble in polar substances.
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In a covalent molecular compound, the attraction between molecules tends to be strong.
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Polarity: polar covalent bond
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Polarity: ionic bond
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Polarity: Difference of 1.7
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Symbol for the less negative atom in a polar covalent bond?
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A nonpolar covalent bond is one that?
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Molecules containing only polar covalent bonds?
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What factor other than electronegativity determines whether a molecule as a whole is polar or not?
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Best description of the compound of water, H2O?
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Best description of the compound of tetrachloride, CCl4?
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A molecule of ammonia, NH3, is?
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Study Notes
Covalent Bonding Fundamentals
- A covalent bond forms when atoms share electrons, creating an attachment.
- Exothermic reactions occur when dissociation energy is released in covalent bonding.
- Atoms bonded through electron sharing result in a molecule.
Bond Types
- A sigma bond is characterized by shared electrons centered between two atoms.
- A pi bond arises from the overlap of parallel orbitals in covalent bonding.
Common Molecular Forms
- Hydrogen, nitrogen, and oxygen typically exist as diatomic molecules (2 atoms).
Bonding Characteristics
- In a double covalent bond, a total of four electrons are shared.
- Bond length refers to the distance between the nuclei of two bonded atoms.
- Generally, the relationship between bond length and strength is shorter bonds are stronger.
Naming Compounds
- Binary molecular compounds consist of nonmetals only, not metals.
- The second element in a binary compound name typically ends with the suffix -ide, not -ite.
- The prefix "tetra-" indicates four atoms, while "hexa-" indicates six.
- "Mono-" is not used for the first element in a compound name.
- For binary acids, the prefix "hydro-" is used for the hydrogen component.
- Oxyacids contain at least three elements, contradicting the idea that they have only two.
Notable Chemical Compounds
- CO is carbon monoxide.
- CO2 is carbon dioxide.
- H2CO3 is carbonic acid.
- NH3 is ammonia.
- N2O4 is dinitrogen tetroxide.
- HNO2 is nitrous acid.
- HNO3 is nitric acid.
- HBr is hydrobromic acid.
- HBrO3 is bromic acid.
Molecular Geometry and Structure
- A structural formula illustrates the arrangement of atoms in a molecule.
- The central atom in a molecule is not necessarily the one with the highest electron affinity.
- In molecules, hydrogen is usually a terminal atom and does not serve as a central atom.
- The number of bonding pairs does not equal the number of electrons but is determined by electron arrangements.
Electron Availability and Resonance
- Calculate total electrons available for bonding in a positive ion by subtracting the charge from total valence electrons.
- A coordinate covalent bond involves electrons donated by only one atom.
- Resonance occurs when multiple valid Lewis structures can be drawn for a molecule.
- An example of resonance can be seen in the nitrate ion.
Specific Molecule Characteristics
- O3 has more than one valid Lewis structure.
- BF3 has fewer than eight electrons around its central atom.
- NO has an odd number of valence electrons.
- SF6 has more than eight electrons around its central atom.
- The VSEPR model determines molecular shapes based on electron pair repulsion.
Bonding Models and Hybridization
- Bond angle is formed between two terminal atoms and the central atom in a molecule.
- The VSEPR model is founded on the principle that shared and unshared electron pairs repel each other.
- A tetrahedral molecule has a central atom with four pairs of bonding electrons.
- A linear molecule features two covalent single bonds with no lone pairs on the central atom.
- A trigonal pyramidal molecule consists of three single covalent bonds and one lone pair on the central atom.
- Hybridization creates new orbitals from the rearrangement of valence electrons, commonly involving carbon.
Electronegativity
- Electronegativity is the atom's ability to attract electrons.
- Fluorine has the highest electronegativity at 3.98.
- Francium has the lowest electronegativity at 0.7.
- Halogens (Group 7A) have the highest overall electronegativities while alkali metals (Group 1A) show the lowest.
Polarity and Molecular Behavior
- Ionic compounds typically dissolve in polar substances.
- In covalent molecular compounds, intermolecular attractions tend to be weak.
- A polar covalent bond features unequal sharing of electrons.
- An ionic bond forms between atoms with significantly differing electronegativities.
- An electronegativity difference of 1.7 often separates covalent and ionic bonding.
- Nonpolar covalent bonds have electrons shared equally.
- Molecules containing only polar covalent bonds can be polar or nonpolar based on molecular geometry.
Specific Molecular Descriptions
- Water (H2O) is described as polar overall, possessing polar covalent bonds.
- Tetrachloride (CCl4) is nonpolar despite having polar covalent bonds.
- Ammonia (NH3) is polar due to its geometry and electronegativity differences.
Studying That Suits You
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Description
Test your knowledge of covalent bonding concepts with this flashcard quiz based on Chapter 8 of the McGraw Hill textbook. Explore important terms like covalent bonds, molecules, and exothermic reactions to enhance your understanding of how atoms interact through electron sharing.