Chemistry Valence Electrons and Bonding Quiz

<p>They are attracted to each other because of opposite charges. (C)</p> Signup and view all the answers

<p>Triple bond (B)</p> Signup and view all the answers

<p>Bromine (A)</p> Signup and view all the answers

<p>They involve the sharing of electrons between atoms. (D)</p> Signup and view all the answers

<p>N2, O2, H2 (C)</p> Signup and view all the answers

<p>Ionic bond (A)</p> Signup and view all the answers

<p>Nonpolar covalent bond (A)</p> Signup and view all the answers

<p>1.9 (A)</p> Signup and view all the answers

<p>Unequally between unlike atoms (B)</p> Signup and view all the answers

<p>A cation (B)</p> Signup and view all the answers

<p>Bonding electrons available for bonding (C)</p> Signup and view all the answers

<p>Involves attractive forces between charged ions (B)</p> Signup and view all the answers

<p>Negative (C)</p> Signup and view all the answers

<p>Crystal lattice structure with oppositely charged ions (A)</p> Signup and view all the answers

<p>Breaking ionic bonds requires significant energy (D)</p> Signup and view all the answers

<p>Closely packed structures with mobile electrons (B)</p> Signup and view all the answers

<p>They have low melting points and lack hardness (D)</p> Signup and view all the answers

<p>They are hard and brittle with high melting points (A)</p> Signup and view all the answers

<p>London dispersion forces (B)</p> Signup and view all the answers

<p>They can move freely and act as a 'negative glue' (B)</p> Signup and view all the answers

<p>Silicon carbide (D)</p> Signup and view all the answers

<p>6 (C)</p> Signup and view all the answers

<p>8 (B)</p> Signup and view all the answers

<p>Bonding electrons (B)</p> Signup and view all the answers

<p>Argon (C)</p> Signup and view all the answers

<p>Two electrons occupying the same orbital (A)</p> Signup and view all the answers

<p>3 (B)</p> Signup and view all the answers

<p>Can hold a maximum of 2 electrons (C)</p> Signup and view all the answers

<p>3 lone pairs and 1 bonding electron (A)</p> Signup and view all the answers

<p>The nonmetal acquires a net negative charge and the metal a net positive charge. (C)</p> Signup and view all the answers

<p>The atom that can form the most bonds. (C)</p> Signup and view all the answers

<p>8 (C)</p> Signup and view all the answers

<p>A pair of bonding electrons. (D)</p> Signup and view all the answers

<p>4 (B)</p> Signup and view all the answers

<p>C2H4 (D)</p> Signup and view all the answers

<p>They require a systematic approach to fit the electrons together. (C)</p> Signup and view all the answers

<p>Two electrons. (C)</p> Signup and view all the answers

<p>The molecular shape and the dipole moment cancellation (D)</p> Signup and view all the answers

<p>Dipole-dipole forces (A)</p> Signup and view all the answers

<p>London dispersion forces (D)</p> Signup and view all the answers

<p>Angular shape with non-canceling dipoles (A)</p> Signup and view all the answers

<p>Due to differences in electronegativities and charge separation (C)</p> Signup and view all the answers

<p>They are weaker forces that operate between molecules (D)</p> Signup and view all the answers

<p>The shape of the molecule and equal electronegativity of atoms (C)</p> Signup and view all the answers

<p>Van der Waals forces (A)</p> Signup and view all the answers

Electron pairing occurs when two electrons occupy the same orbital.

The outermost energy level of an atom, containing electrons involved in bonding.

An element with properties of both metals and nonmetals, located near the dividing line on the periodic table.

Bond formed by the electrostatic attraction between a positive ion and a negative ion.

Bond formed by the sharing of electrons between two atoms.

Covalent bond where one pair of electrons is shared between two atoms.

Covalent bond where two pairs of electrons are shared between two atoms.

Elements that naturally exist as molecules containing two atoms of the same element.

Crystals where ions form a lattice structure, held together by electrostatic attraction.

Crystals formed by metals, characterized by mobile valence electrons holding positive ions together.

Crystals where molecules are arranged in a regular lattice, held together by weak intermolecular forces.

Crystals composed of atoms connected by a continuous network of covalent bonds resulting in high melting points and hardness

The regular, repeating arrangement of ions or molecules in a crystal.

Indicates strong bonds between particles, requiring significant energy to break.

Ionic compounds conduct electricity when molten or dissolved in water because ions are free to move.

The ions arrange themselves in a structure where they are always surrounded by oppositely charged ions preventing the lattice from moving around freely.

A chemical bond formed by the sharing of electrons between atoms.

A chemical bond formed by the transfer of electrons from one atom to another, resulting in oppositely charged ions.

A measure of an atom's ability to attract electrons in a chemical bond.

A covalent bond in which electrons are shared unequally between atoms due to differences in electronegativity.

A covalent bond in which electrons are shared equally between atoms due to similar electronegativity values.

Metals lose electrons to form positive ions (cations), while nonmetals gain electrons to form negative ions (anions). These oppositely charged ions are strongly attracted to each other.

The difference in electronegativity values helps predict the type of bond (ionic, polar covalent, or nonpolar covalent) that will form between two atoms.

Linus Pauling explained that bond polarity is determined by the electronegativity difference between the bonded atoms.

Electrons in an atom's outermost energy level that are involved in chemical bonding.

Oxygen has 6 valence electrons.

Argon has eight valence electrons.

Chlorine has 7 valence electrons.

Represent atoms by showing ONLY their valence electrons as dots.

Atoms tend to gain, lose, or share electrons to achieve a full valence shell of 8 electrons(with exceptions).

Regions in space where valence electrons may be found.

A maximum of 8 electrons can occupy the valence energy level.

Electrons move from a metal to a nonmetal, creating a positive charge on the metal and a negative charge on the nonmetal.

Visual representations of valence electrons in atoms and molecules using dots placed around the element symbols.

Outermost electrons in an atom that are involved in bonding.

Chemical bonds formed when atoms share electrons.

Represent chemical structures using lines to indicate covalent bonds between atoms.

Another way to represent covalent molecules using dots to show valence electrons and lines to show bonding pairs.

The tendency of an atom to form chemical bonds with other atoms.

The atom with the highest bonding capacity is generally placed in the center of a Lewis structure.

A molecule with an overall charge separation, one end positive and the other negative, resulting from an unequal sharing of electrons.

A molecule with no net charge separation, meaning there's no significant overall polarity.

The weak forces or bonds between molecules.

Attractive forces between the positive end of one polar molecule and the negative end of another.

Weak intermolecular forces present in ALL molecules, caused by temporary fluctuations in electron distribution creating temporary dipoles.

A quantitative measure of the polarity of a molecule.

A measure of an atom's ability to attract electrons towards itself in a chemical bond.

A separation of charge in a bond due to differences in electronegativity of atoms.