問題一覧
1
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
2
An object that has motion.
Keeps the particles
at a distance and/or moving
around.
KINETIC ENERGY
3
IMEs are attractive forces between molecules.
It pulls the particles together.
INTERMOLECULAR FORCES
4
is the tendency of certain matter or object to change its shape as a response to change in temperature.
THERMAL EXPANSION
5
Have definite volume but no definite shape
Flow and takes the shape of their container
• Very difficult to compress
• Slightly expand when heated
Liquids
6
Have definite volume and shape
• Do not flow
• Virtually
incompressible
• Expands when heated, but to a lesser extent than liquids and gasses
Solids
7
• Have definite volume but no definite shape
• Flow and takes the shape of their container
• Very difficult to compress
• Slightly expand when heated
Liquids
8
•Strongly attracted to each other
• Vibrate in fixed position
• Vibrate faster when heated
Solids
9
Weakly attracted to each other;break their
• Vibrate in fixed position
interaction easily
• Vibrate faster when heated
Liquid
10
an atom or
molecule that is charged due to a
difference in the number of electrons and protons.
IONS
11
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
12
Exists only in molecules that contain a hydrogen atom bonded to a highly electronegative atom.
Hydrogen Bonds
13
•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
14
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
15
Constantly moving/stable. (stable - 8 electrons)
NEUTRAL ATOMS
16
imbalance of neutrons.
TEMPORARY DIPOLE
17
attracted charges from neutral to temporary.
INDUCED DIPOLE
18
refers to cleanliness of a certain substance not contaminated with any other foreign substances.
Purity
19
Pressure exerted by its vapor when in equilibrium with its liquid or solid. It is the liquid's tendency to evaporate
Vapor Pressure
20
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
21
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
22
Temperature at which a liquid boils.
Boiling point is affected by two different factors:
Pressure & Purity.
Boiling Point
23
defined by the amount of enthalpy (heat energy) that is required to transform a liquid substance into a gas or vapor.
Heat Of Vaporization
24
• 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
25
• 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
26
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
27
• The crystals consisting of molecules, which are held together through Van der Waals' forces, are called molecular crystals.
Molecular Solid
28
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
29
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
30
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
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問題一覧
1
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
2
An object that has motion.
Keeps the particles
at a distance and/or moving
around.
KINETIC ENERGY
3
IMEs are attractive forces between molecules.
It pulls the particles together.
INTERMOLECULAR FORCES
4
is the tendency of certain matter or object to change its shape as a response to change in temperature.
THERMAL EXPANSION
5
Have definite volume but no definite shape
Flow and takes the shape of their container
• Very difficult to compress
• Slightly expand when heated
Liquids
6
Have definite volume and shape
• Do not flow
• Virtually
incompressible
• Expands when heated, but to a lesser extent than liquids and gasses
Solids
7
• Have definite volume but no definite shape
• Flow and takes the shape of their container
• Very difficult to compress
• Slightly expand when heated
Liquids
8
•Strongly attracted to each other
• Vibrate in fixed position
• Vibrate faster when heated
Solids
9
Weakly attracted to each other;break their
• Vibrate in fixed position
interaction easily
• Vibrate faster when heated
Liquid
10
an atom or
molecule that is charged due to a
difference in the number of electrons and protons.
IONS
11
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
12
Exists only in molecules that contain a hydrogen atom bonded to a highly electronegative atom.
Hydrogen Bonds
13
•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
14
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
15
Constantly moving/stable. (stable - 8 electrons)
NEUTRAL ATOMS
16
imbalance of neutrons.
TEMPORARY DIPOLE
17
attracted charges from neutral to temporary.
INDUCED DIPOLE
18
refers to cleanliness of a certain substance not contaminated with any other foreign substances.
Purity
19
Pressure exerted by its vapor when in equilibrium with its liquid or solid. It is the liquid's tendency to evaporate
Vapor Pressure
20
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
21
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
22
Temperature at which a liquid boils.
Boiling point is affected by two different factors:
Pressure & Purity.
Boiling Point
23
defined by the amount of enthalpy (heat energy) that is required to transform a liquid substance into a gas or vapor.
Heat Of Vaporization
24
• 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
25
• 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
26
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
27
• The crystals consisting of molecules, which are held together through Van der Waals' forces, are called molecular crystals.
Molecular Solid
28
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
29
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
30
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