# data[].attributes.body
1. ionic compounds such as NaC/ is soluble in water

2. Ionic compounds such as NaC/ are insoluble in organic solvents such as ethanol

# data[].attributes.body
1. negatively charged chlorine anions

positively charged sodiums cations

2. molten and aqueous

# data[].attributes.body
When melting, the electrostatic forces of attraction between the ions is overcame by thermal energy of the particles and when sodium chloride was dissolved in water, the ionic bond between the particles breaks as the sodium and chlorine particles are pulled apart by the water molecules

# data[].attributes.body
Molten: substance that is in liquid form

Aqueous: when its dissovles in water

Solid state. it lit up in molten and aqueous state

# data[].attributes.body
1. NaCl has a giant ionic lattice structure.

2. In solid NaCl, cations and anions are vibrating and rotating about their fixed positions. Absence of free moving sodium cations and chloride anions. They are attracted by strong electrostatic forces of attraction.

3. In molten and aqueous states, cations and anions are sliding past each other. Presence of free moving sodium cations and chloride anions. They are not attracted by strong electrostatic forces of attraction.

# data[].attributes.body
1. NaCl has a giant ionic lattice structure

2. In solid NaCl, cations and anions are no free moving charged particles. absence of free moving charged articles.

why are they NOT moving? Strong electrostatic forces.

3. In molten and aqueous states, can conduct electricity

Presence of free moving __ions__

why are they moving?

The ions are overcoming electrostatic forces. what happen to the structure? The structure breaks apart

# data[].attributes.body
1 . NaCl has a giant ionic lattice structure.

2. In solid NaCl, there is an absence of free moving sodium cations and chloride anions as they are held by strong electrostatic forces.

3. In molten and aqueous states, there is the presence of free moving sodium cations and chloride anions. Molten and aqueous states have less electrostatic force as they are sliding past one another. This allows the sodium cations and chloride anions to be free moving

# data[].attributes.body
1.NaCl has a giant ionic lattice structure.

2.In solid NaCl,cations and anions are not free moving and they are vibration about their fixed positions

absence of free moving NaCl cations and anions.They are held together by very strong forces of attraction.

3.In molten and aqueous states, the cations and anions are free moving as they are held together by weaker forces of attraction

# data[].attributes.body
1. NaCl has a giant lattice structure

2. In solid NaCl, cations and anions are absence of free moving sodium cation and chlorine anion

3. In molten and aqueous states,

Presence of free moving sodium cation and chlorine anions

# data[].attributes.body
1. NaCl has a giant ionic lattice structure

2. In solid NaCl, there is an absence of free moving sodium cations and chlorine anions as there are strong electrostatic forces.

3. In molten and aqueous states, there is presence of free moving cations and anions as there is weaker electrostatic forces

# data[].attributes.body
1. NaC/ has a giant ionic lattice structure

2. In solid NaC/, there is an absence of free moving sodium cations and Chlorine anions

3. In molten and aqueous states, there is a presence of free moving ions

# data[].attributes.body
Nacl has a giant ionic lattice structure. In solid NaCl there are no free moving electrons. In molten and aqueous state there is a presence of free moving electrons

# data[].attributes.body
1. Ionic compounds are soluble in water

2. Ionic compounds are soluble in organic solvent

# data[].attributes.body
1. NaCl has a giant ionic lattice structure.

2. In solid NaCl, cations and anions are not free moving. There is an absence of sodium cations and chloride anions.

3. In molten and aqueous states, there is a presence of free moving sodium cations and chloride anions.

# data[].attributes.body
1. NaCl has a giant ionic lattice structure

2. In solid NaCl, cations and anions are

# data[].attributes.body
1. Positively charged sodium cations and negatively charged chloride anions

2. Molten and aqueous

# data[].attributes.body
1. Sodium cation and chloride anion

2. molten and aqueous

# data[].attributes.body
When melted, strong electrostatic forces of attraction are overcome. When dissolved in water, the water molecules pulls apart the crystal.

# data[].attributes.body
1. Molten: refers to a substance in the liquid state

Aqueous: refers a substance dissolved in water

2. It lit up in the aqueous and molten state but not in the solid state.

# data[].attributes.body
1. Ionic compounds are soluble in water.

2. Ionic compounds are insoluble in organic solvent.

# data[].attributes.body
1. NaCl has a giant ionic lattice structure

2. In solid NaCl, cations and anions are absence of free moving sodium and chlorine ions it has strong electrostatic forces of attraction between sodium cation and chloride anions.

3. In molten and aqueous states, presence of free moving sodium and chlorine ions, because

# data[].attributes.body
1. positively charged sodium ions and negatively charged chloride ions

2. molten and aqueous

# data[].attributes.body
When sodium chloride melted, the forces of attraction between the particles are overcome. However, when the sodium chloride is dissolved in water, it is pulled apart by water molecules.

# data[].attributes.body
1. aqueous solution is a solution with water as a solvent. Molten is simply an object that has been melted or liquefied by heat.

2. It lit up when it is molten but it did not lit up when it is in the solid state.

# data[].attributes.body
Ionic compounds are soluble in water

Ionic compounds are insoluble in organic solvent

# data[].attributes.body
NaCl has a giant lattice structute structure

In solid NaCl, there are no free moving sodium cations and chlorine anions.

In molten and aqueous states, there are free moving sodium cations and chlorine anions

# data[].attributes.body
1. Sodium cation and chloride anion.

2. Molten and aqueous.

# data[].attributes.body
When melted, sodium chloride gains thermal energy and overcomes its strong electrostatic forces of attraction between sodium and chloride particles. When dissolved, the sodium and chloride particles were pulled apart by water molecules.

# data[].attributes.body
1. Molten sodium chloride is when it is in a liquid state and aqueous sodium chloride is when it is dissolved in water.

2. The bulb lit up when sodium chloride was molten and in liquid form and also lit up when it was dissolved in water. It did not light up in its solid state.

# data[].attributes.body
1)NaCl has a giant lattice structure.

2)In solid NaCl, cations and anions are stationary at its fixed position. There is an absence of free moving electrons.

3)In molten and aqueous states, there is presence of free moving electrons.

# data[].attributes.body
1. Na+ (sodium)

2. molten and aqueous

# data[].attributes.body
1)The charged particles are sodium cation and chloride anion

2)In aqueous state the particles are mobile

# data[].attributes.body
1)Ionic compounds are soluble in water

2)Ionic compounds are insoluble in organic solvent

# data[].attributes.body
The structure of sodium chloride is no longer being held by a very strong electrostatic force

# data[].attributes.body
Structure: giant ionic lattice

In solid NaCl, there is absence of free moving cations and anions as they are vibrating about fixed positions, since there are strong electrostatic forces of attraction.

In molten and aqueous NaCl, there is presence of free moving cations and anions, as the giant lattice structure

Solid NaCl cannot conduct electricity. Molten and aqueous NaCl can conduct electricity. The high amounts of mobile ions allow for it to conduct electricity.

# data[].attributes.body
1. I can understand that 'molten' is the product of a salt (in this case, sodium chloride) being heated and melting from a solid to a liquid, whereas 'aqueous' is the result of a salt (sodium chloride) dissolving in a solvent (water)

2. Part #1; the bulb did not light up when sodium chloride was in its solid state, but it lit up when it was melted and turned into a liquid.

Part #2; the bulb did not light up when there was just water and only lit up when sodium chloride was put into the water (and grew brighter when in contact with more sodium chloride)

# data[].attributes.body
-When melting, the sodium chloride particles gain thermal energy and overcome electrostatic forces between the sodium cations and chloride anions.

-When dissolved in water, the sodium chloride particles are pulled apart by the water molecules

# data[].attributes.body
1.Ionic compounds are soluble in water

2.Ionic compounds are insoluble in organic solvent

# data[].attributes.body
NaCl has a giant ionic lattice structure

In solid NaCl, there are no free moving sodium cations and chloride anions.

In molten and aqueous states, there are free moving sodium cations and chloride anions.

# data[].attributes.body
1.Sodium cation and chloride anion

2.molten and aqueous

# data[].attributes.body
When sodium chloride melts, it overcomes electrostatic forces of attraction between sodium cation and chloride anion. When sodium chloride dissolves in water, it is being pulled apart by the water molecules

# data[].attributes.body
1) I understand that

-Molten: meant that the element or compound has been melted into a liquid form at very high temperature.

-Aqueous: meant a substance that is dissolved

2)The bulb lit up when sodium chloride was at molten and aqueous state but didn't lit up at solid state

# data[].attributes.body
1.Molten means the liquid state of something that is solid in room temperature. Aqueous means that the substance is dissolved in water.

2.The light bulb lit up when the sodium chloride was molten and aqueous, while the bulb did not light up when the sodium chloride was in solid state

# data[].attributes.body
When sodium chloride was melting, sodium cations and chloride anions gained thermal energy to overcome strong electrostatic forces of attraction between sodium cations and chloride anions.

# data[].attributes.body
1. Molten sodium chloride is when sodium chloride melts and changes to a liquid while aqueous sodium chloride is sodium chloride dissolved in water making sodium chloride solution.

2. The bulb lit up when sodium chloride was in the liquid stage and when dissolved in water. The bulb did not light up when sodium chloride was in solid state.

# data[].attributes.body
1. Sodium

2. Molten and aqueous

# data[].attributes.body
1. Melted: The sodium chloride particles gain thermal energy to overcome strong electrostatic forces of attraction when heated.

Dissolved: The particles of water bond with the particles of sodium chloride, slowly pulling them apart and dissolving sodium chloride into the solvent.

# data[].attributes.body
1. Molten: the liquid form of a solid that is melted down

Aqueous: a substance dissolved in water

2. It lit up when it was molten and aqueous but not in it's solid state

# data[].attributes.body
1. Ionic compounds such as NaCl are soluble in water.

2. Ionic compounds such as NaCl are insoluble in organic solvents such as ethanol.

# data[].attributes.body
1. NaCl has a giant ionic lattice structure.

2. In solid NaCl, there is an absence of free moving sodium and chlorine ions.

3. In molten and aqueous states, there is no absence of free moving ions.

# data[].attributes.body
1. NaCl has a ____________ structure

2. In solid NaCl, cations and anions are ____

Presence / absence of free moving ______

why are they NOT moving?

3. In molten and aqueous states, ______

Presence / absence of free moving ______

why are they moving? what happen to the structure?

# data[].attributes.body
1. Negatively charged chlorine anions and positively charged sodium cations.

2. Molten and aqueous.

# data[].attributes.body
When sodium chloride was melted, the thermal energy it gained overcame the strong FoA between the NaCl particles, while when sodium chloride was dissolved in water, the ionic bond between the particles breaks as the sodium and chlorine particles are pulled apart by the water molecules.

# data[].attributes.body
1. Molten sodium chloride is when sodium chloride is in its liquid form. Aqueous sodium chloride is when the sodium chloride is dissolved in water and forms sodium chloride solution.

2. The bulb lit up when NaCl was in molten and aqueous state, but did not light up when it was in solid state.

# data[].attributes.body
A lattice structure is a three-dimensional arrangement of ions or atoms.

Giant structure meant they are made up of large numbers of the same ions arranged in a repeated pattern.

# data[].attributes.body
1. solid

2. The particles are very closely packed and orderly arranged.

# data[].attributes.body
1. When going through the process of melting the electrostatic forces of attraction were overcome by the thermal energy of the particles and when dissolved, the particles were pulled apart by the particles of the solvent

# data[].attributes.body
1. I can understand from the video that molten refers to the sodium chloride mixture in its liquid form and aqueous refers to it when it is dissolves in water

2. Molten and aqueous. It did not light up in solid state

# data[].attributes.body
The physical state of the ionic compounds such as sodium chloride and magnesium oxide have a melting point of 801 and 2852 degrees celsius and since room temperature is below those temperature they will be in the solid state.

# data[].attributes.body
When a substance is heated, it gains thermal energy. According to Figure 2.2, the lines between the lattice structure of NaCl, which represent the strong electrostatic forces of attraction between the particles, start to fade as the compound is heated. This shows that as the compound gains thermal energy, it overcomes the electrostatic forces of attraction between its particles.

# data[].attributes.body
According to Figure 2.1, the ionic compounds NaCl and MgO will be in solid state at room temperature as both of their melting points are above room temperature. (NaCl has a melting point of 801 degrees Celsius while MgO has a melting point of 2852 degrees Celsius.)

# data[].attributes.body
The physical state of ionic compounds at room temperature is solid. Fig 2.1 shows that the melting point of sodium chloride is 801 degrees Celsius and the melting point of magnesium oxide is 2852 degrees Celsius. This means that at room temperature, sodium chloride and magnesium oxide are solids.

# data[].attributes.body
1. Ionic bonding refers to the strong electrostatic forces between positively charged cations and negatively charged anions.

2. The lines refer to the strong electrostatic forces of attraction between the particles cations and anions.

# data[].attributes.body
Ionic compounds require a larger amounts of thermal energy in order to overcome the strong electrostatic forces of attraction between the cation and anion

# data[].attributes.body
ionic compounds have high melting points because they have strong electrostatic forces of attraction between the cations and anions. they need a high amount of thermal energy in order to melt

# data[].attributes.body
As the ionic bond have strong electrostatic forces of attractions between the sodium cations and chlorine anions need a large amount of thermal energy to overcome the strong electrostatic forces of attraction between the cations and anions

# data[].attributes.body
Ionic compounds require a large amount of thermal energy to overcome strong electrostatic forces of attraction between cations and anions.

# data[].attributes.body
As ionic compounds have very strong electrostatic FoA between its anions and cations, more energy (thermal specifically) is required to overcome the forces.

# data[].attributes.body
Ionic compounds have strong electrostatic forces of attraction between cations and anions. It requires more energy to overcome strong electrostatic forces of attraction.

# data[].attributes.body
Ionic compounds have very strong electrostatic forces of attraction between cations and anions which requires a lot of thermal energy to overcome the electrostatic force of attraction

# data[].attributes.body
1. The ionic bond has strong electrostatic forces of attraction between the cations and the anions. This would require a high amount of thermal energy for overcoming the strong electrostatic forces of attraction.

# data[].attributes.body
Ionic compounds such as Sodium Chloride have high electrostatic forces of attraction holding it together. This strong electrostatic force of attraction between the cations and anions in Sodium Chloride holds them together. Since this electrostatic force is very strong, a lot of thermal energy is needed to weaken and destroy this force of attraction. Therefore, more thermal energy is required to melt or boil ionic compounds. This causes them to have high melting and boiling points.

# data[].attributes.body
Ionic bonds have very high melting points because they need large amounts of thermal energy to overcome the very strong electrostatic force of attraction between the cation (metal) and anion (non-metal).

# data[].attributes.body
1. Ionic compounds have very strong electrostatic forces of attraction between cations and anions and needs a large amount of thermal energy to overcome the strong electrostatic forces of attraction between the cations and anions.

# data[].attributes.body
As ionic bond is closely packed in orderly manner, it would have a strong electrostatic forces of attraction between cations and anions Large amount of thermal energy will be needed to overcome the strong electrostatic force. Thus it would have a high melting and boiling point.

# data[].attributes.body
The particles gain thermal energy to overcome strong electrostatic forces of attractions between cations and anions.

# data[].attributes.body
the particles of sodium chloride gain thermal energy and overcome strong electrostatic forces of attraction.

# data[].attributes.body
Sodium chloride gains thermal energy and overcomes forces of attraction to change state from solid to liquid and move further away from one another

# data[].attributes.body
the amount of energy needed to overcome the forces of attraction is very high. The thermal energy gained when NaC/ melts. this helps the particles in the sodium chloride to overcome the strong forces of attraction and the strong electrostatic forces between the chlorine anions and sodium cations, resulting in Sodium chloride to have a high boiling point

# data[].attributes.body
Thermal energy is gained to overcome attractive forces. The particles change from very closely packed and orderly arranged to closely packed and disorderly arranged.

# data[].attributes.body
1. When sodium chloride melts the particles gain thermal energy which is converted to kinetic energy and the particles begin to vibrate and rotate more vigorously, as a result the particles are able to overcome the forces of attraction and the particles change from orderly arranged and very closely packed to unorderly arranged and closely packed, the particles also change from vibrating and rotating amongst their fixed position to sliding past one another

# data[].attributes.body
When sodium chloride melts, particles gain thermal energy to overcome strong electrostatic forces of attraction between cations and anions.

# data[].attributes.body
1. As sodium chloride gains heat, it gains thermal energy and overcomes strong forces of attraction. It will then change from a solid to a liquid.

# data[].attributes.body
when sodium chloride melts it chanages from being in solid to being in a liquid state, the particles move further away from each other, gain thermal energy and can overcome the forces of attraction between cations and anions

# data[].attributes.body
Thermal energy from the heat is gained for the sodium chloride particles so that they can overcome the very strong forces of attraction (electrostatic) to change its physical state from solid to liquid

# data[].attributes.body
When sodium chloride melts, thermal energy is gained. This helps the particles in sodium chloride overcome the very strong forces of attraction in a solid. After some time, sodium chloride will turn from solid into liquid.

# data[].attributes.body
The particles gain thermal energy and can overcome the forces of attraction.

# data[].attributes.body
1. an ionic bond is the transfer of electrons from metals to non-metals so that they can achieve octet/duplet structure and stable noble gas configuration. It forms a very strong electrostatic attraction. For example, sodium is a metal with a configuration of 2.8.1 and it loses 1 electron to form a noble gas configuration and become Na+. C/ is not a metal and has a electronic configuration of 2.8.7 and it gains 1 electron from sodium and therefore become C/+, achieving a stable noble gas configuration

2. the lines are strong ionic bonds and are strong electrostatic FOA

# data[].attributes.body
1. strong electrostatic bonds due to transfer of electrons in ionic bonding

# data[].attributes.body
1. The ionic bond in sodium chloride refers to strong electrostatic forces of attraction between the 2 particles, sodium and chlorine. This is possible as attraction occurs between a positive and negative charge as a result when forming an ionic compound The positive - charged Sodium, cation with a charge of + is attracted to the negatively charged chlorine anion which has a charge of -.

2. It may be the electro static forces of attraction

# data[].attributes.body
1)The ionic bond happens when one sodium electron is transferred to the chlorine atom forming a strong electrostatic force of attraction between cations and anions.

2)The forces of attraction

# data[].attributes.body
Q1: A sodium atom, has a valence electron of 1. A chlorine atom has 7 valence electrons. Therefore, when a sodium and chlorine atom bond, the sodium atom transfers 1 electron the chlorine atom which causes the sodium atom to be a sodium cation with a charge of +1, and the chlorine atom to be a anion with a charge of -1. After bonding, both Sodium and Chlorine attain a noble gas configuration. Since sodium is a metal, and chlorine is a non-metal, the bond that is formed is called an ionic bond.

Q2: The black line represent the strong electrostatic forces while the dotted lines represent the ionic bonds between the molecules.

# data[].attributes.body
1. Ionic bonds are the bonds formed when atoms of a metal transfer electrons to atoms of a non-metal to form cations and anions. The cations and anions are held together by strong electrostatic forces of attraction.

2. The lines represent the electrostatic forces.

# data[].attributes.body
1. ionic bond is where a cation transfers electrons to an anion to attain a net 0 charge

2. the lines show the electrostatic foa between the cation and the anion

# data[].attributes.body
1. Ionic bond is a transfer of electrons between a metal and non-metal with strong electrostatic forces of attraction. NaCl, Na is a metal which loses elections to form a cation and Cl is a non-metal which gains electrons to form an anion.

2. it shows the electrostatic forces

# data[].attributes.body
1. There are strong electrostatic forces of attraction between sodium cation and chlorine anion.

2. electrostatic force

# data[].attributes.body
1. An ionic bond is made up of a metal and a non-metal; sodium (metal) and chlorine (non-metal). The particles are being held by a very strong electrostatic force of attraction between cations (sodium ion) and anions (chlorine ion).

2. The figure being three-dimensional

# data[].attributes.body
ionic bonding is when sodium choride atom transfers 1 valence electron to chlorine.They are held together by very strong elclectrostatic forces of attraction.

# data[].attributes.body
1.A strong electrostatic force of attraction between sodium cation and chloride anion.

2.The electrostatic force

# data[].attributes.body
1. ionic bonding is when a metal and a non-metal become cations and anions. the electrostatic force causes the ions to be attracted to one another.

2. It represents the electrostatic force