gen chem exam

30問 • 1年前

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Explains the properties of solids and liquids in terms of the intermolecular forces of attraction and the kinetic energy of the individual particles

KINETIC MOLECULAR MODEL

An object that has motion. Keeps the particles at a distance and/or moving around.

KINETIC ENERGY

IMEs are attractive forces between molecules. It pulls the particles together.

INTERMOLECULAR FORCES

is the tendency of certain matter or object to change its shape as a response to change in temperature.

THERMAL EXPANSION

Have definite volume but no definite shape Flow and takes the shape of their container • Very difficult to compress • Slightly expand when heated

Liquids

Have definite volume and shape • Do not flow • Virtually incompressible • Expands when heated, but to a lesser extent than liquids and gasses

Solids

• Have definite volume but no definite shape • Flow and takes the shape of their container • Very difficult to compress • Slightly expand when heated

Liquids

•Strongly attracted to each other • Vibrate in fixed position • Vibrate faster when heated

Solids

Weakly attracted to each other;break their • Vibrate in fixed position interaction easily • Vibrate faster when heated

Liquid

an atom or molecule that is charged due to a difference in the number of electrons and protons.

IONS

Exist between polar molecules. Polar substances are those that posseses a permanent difference dipole moment attributed to the difference electronegativities of their component atoms and how these are arranged in space.

DIPOLE- DIPOLE FORCES

Exists only in molecules that contain a hydrogen atom bonded to a highly electronegative atom.

Hydrogen Bonds

•Acts between an ion (either positive or negative) and a polar molecule. • The degree of ion-dipole interaction depends on the size and charge of the ion, on the size, and on the dipole moment of the polar molecule.

ION-DIPOLE FORCES

Exist between all atoms and molecules. These are the only forces that exist in everything. They arise from the continuous movement of electrons in particles.

LONDON DISPERSION FORCES

Constantly moving/stable. (stable - 8 electrons)

NEUTRAL ATOMS

imbalance of neutrons.

TEMPORARY DIPOLE

attracted charges from neutral to temporary.

INDUCED DIPOLE

refers to cleanliness of a certain substance not contaminated with any other foreign substances.

Purity

Pressure exerted by its vapor when in equilibrium with its liquid or solid. It is the liquid's tendency to evaporate

Vapor Pressure

Property of a liquid to resist external force and thus assume a lesser surface area. Atoms on the surface are attracted to one side. Atoms in the middle are attracted equally in all directions.

Surface Tension

Resistance of a liquid to flow. Referred to as the thickness or thinness of a liquid There are two types of level of viscosity: (1) high viscosity (high resistance) and (2) low viscosity (low resistance)

VISCOSITY

Temperature at which a liquid boils. Boiling point is affected by two different factors: Pressure & Purity.

Boiling Point

defined by the amount of enthalpy (heat energy) that is required to transform a liquid substance into a gas or vapor.

Heat Of Vaporization

• Consists of particles that are arranged in a three-dimensional manner. The intermolecular forces between them are equal. Arrangement is aligned and rigid.

CRYSTALLINE SOLID

• refers to being shapeless. Have an irregular arrangement of solid particles. The intermolecular forces between them are not equal. • Vibration is not fixed.

AMORPHOUS SOLID

are those crystalline solids in which the particles forming the crystal are positively and negatively charged ions, held together by strong electrostatic forces of attraction (attract/repulse. Has a high IMF and stable/ maximum stability.) Attraction depends on particles' size and charge. High boiling and melting point, low volatility

Ionic Solid

• The crystals consisting of molecules, which are held together through Van der Waals' forces, are called molecular crystals.

Molecular Solid

formed by metal atoms (Ex.: Aluminum, Iron, Silver). The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a "sea" of delocalized electrons (attracted to positive-charged ion. Only atoms outside can go anywhere). • The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.

Metallic Solid

are formed by networks or chains of atoms or molecules held together by covalent bonds forming a continuous three-dimensional structure. This results in a strong and rigid solid with high melting and boiling points.

Covalent Network solids

If one end of the molecule has a positive charge while the other end has a negative charge, the molecule is polar. The molecule then is said to be a ____.

Polar Molecule

Gen Chem

Joshua Timbol · 65問 · 2年前

Gen Chem