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What is an ion?
An ion is a charged particle that has either lost or gained electrons.
What is an ionic bond?
An ionic bond is formed by the transfer of electrons from one atom to another, resulting in the attraction between positively and negatively charged ions.
How are ions formed?
Ions are formed by the loss or gain of electrons.
What is the charge of a cation?
Cations have a positive charge.
What is the charge of an anion?
Anions have a negative charge.
How do ions achieve stability?
Ions achieve stability by attaining a noble gas electron configuration.
What is the difference between cations and anions?
Cations are positively charged ions, while anions are negatively charged ions.
What is an example of an ionic compound?
Sodium chloride (NaCl) is an example of an ionic compound.
How is an ionic bond formed?
An ionic bond is formed through the transfer of electrons from a metal to a non-metal.
What is electronegativity?
Electronegativity is the tendency of an atom to attract electrons in a bond.
What is a covalent bond?
A covalent bond is formed when electrons are shared between atoms.
How are electrons shared in covalent bonds?
Electrons can be shared equally or unequally in covalent bonds.
What is the difference between ionic and covalent bonds?
Ionic bonds involve the transfer of electrons, while covalent bonds involve the sharing of electrons.
What determines bond polarity?
Bond polarity is determined by the difference in electronegativity values between the bonding atoms.
What is a polar covalent bond?
A polar covalent bond is formed when electrons are shared unequally between atoms.
What is a nonpolar covalent bond?
A nonpolar covalent bond is formed when electrons are shared equally between atoms.
How do you determine bond type?
You determine bond type by examining the difference in electronegativity between the atoms.
What is an example of a polar molecule?
Water (H2O) is an example of a polar molecule.
How do lone pairs affect bond polarity?
Lone pairs can increase the polarity of a molecule by affecting the distribution of electron density.
What determines molecular shape?
Molecular shape is determined by the arrangement of electron pairs around the central atom.
What is the VSEPR theory?
The Valence Shell Electron Pair Repulsion (VSEPR) theory states that electron pairs repel each other to minimize their energy.
What is the shape of CO2?
The shape of carbon dioxide (CO2) is linear.
What is the shape of H2O?
The shape of water (H2O) is bent or angular.
What is the shape of NH3?
The shape of ammonia (NH3) is trigonal pyramidal.
What is the shape of CH4?
The shape of methane (CH4) is tetrahedral.
What is the shape of BF3?
The shape of boron trifluoride (BF3) is trigonal planar.
What is the shape of SF6?
The shape of sulfur hexafluoride (SF6) is octahedral.
What is the shape of NH4+?
The shape of ammonium (NH4+) is tetrahedral.
What is the significance of lone pairs?
Lone pairs affect molecular geometry and can influence bond angles.
What is polarization?
Polarization is the distortion of an electron cloud around a molecule.
What are intermolecular forces?
Intermolecular forces are the forces of attraction or repulsion between molecules.
What is the strongest intermolecular force?
Hydrogen bonding is the strongest intermolecular force.
What is the weakest intermolecular force?
London dispersion forces are the weakest intermolecular force.
What is the force between polar molecules?
The force between polar molecules is dipole-dipole attraction.
What is the force between nonpolar molecules?
The force between nonpolar molecules is London dispersion forces.
What is an example of London dispersion forces?
London dispersion forces are found in hydrocarbons and noble gases.
What is an example of dipole-dipole forces?
Water (H2O) exhibits dipole-dipole forces.
What is an example of hydrogen bonding?
Hydrogen bonding occurs when hydrogen is attached to nitrogen, oxygen, or fluorine.
What affects the strength of intermolecular forces?
Molecular polarity and size affect the strength of intermolecular forces.
What is metallic bonding?
Metallic bonding is the sharing of delocalized electrons among a lattice of metal cations.
What are properties of metals?
Properties of metals include high conductivity, malleability, and ductility.
What is the significance of delocalized electrons?
Delocalized electrons contribute to the conductivity and malleability of metals.
What is the relationship between metallic bonding and conductivity?
Metallic bonding allows for high conductivity in metals due to the free movement of electrons.
What is the relationship between metallic bonding and malleability?
Metallic bonding provides malleability as layers of atoms can slide past each other.
How do metallic bonds contribute to ductility?
Metallic bonds allow metals to be stretched into wires without breaking.
What is the difference between pure metals and alloys?
Pure metals consist of one type of metal atom, while alloys contain more than one type of metal.
What is the effect of alloying on properties?
Alloying can alter properties for specific purposes, enhancing strength or corrosion resistance.
What is the significance of lattice structure in metals?
The lattice structure in metals influences their physical properties, including melting and boiling points.
How do metallic bonds affect melting and boiling points?
Metallic bonds generally contribute to high melting and boiling points in metals.
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