Acids and ases first quiz Flashcards

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1
Q

What is empirical ?

A

Empirical refers to knowledge or information that is based on observable and measurable evidence.

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2
Q

What is theoretical?

A

Based on ideas or concepts that explain something.
It’s more about thinking and understanding how things work, even if you can’t see them directly.

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3
Q

What does matter break down into?

A

Pure substances and mixtures

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4
Q

What do both pure substances and mixtures break down into?

A

Pure substances break down into compounds and elements.
Mixtures break down into homogenous and heterogenous mixtures.

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5
Q

What is a solution empirically and theoretically?

A

Empirically, a solution is homogeneous because its properties are consistent throughout. Theoretically, it is uniform at the atomic and molecular levels.

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6
Q

What is the normal prerequisite for chemical change?

A

dissolving substances

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7
Q

What is a matter?

A

anything that has mass and occupies space

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8
Q

What is uniform in science?

A

In science, when something is described as uniform, it means that its properties, appearance, or composition are identical throughout.

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9
Q

What is a pure substance?

A

Made up of one thing only

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10
Q

What is a compound?

A

substance made up of 2 or more elements

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11
Q

What is an element?

A

Substance made up of only one type of atom

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12
Q

What is a mixture

A

combination of 2 or more substances

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13
Q

What is a homogenous mixture

A

A homogeneous mixture is one where the components are evenly distributed, so it looks the same throughout.

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14
Q

What is a heterogenous mixture

A

A heterogeneous mixture has unevenly distributed components, so you can often see the different parts.

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15
Q

What is the definition of “dissolving”

A

A process in which
Dissolving is the process where a substance (the solute) breaks down and mixes evenly into another substance (the solvent) to form a solution.

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16
Q

What is dissociation

A

Dissociation is the process where a compound breaks apart into smaller particles, such as ions or molecules, when it dissolves in a solvent.

17
Q

WHat is ionization

A

the process by which an electrically charged neutral atom or molecule is converted to an ion, from the loss or gain of electrons

18
Q

H20 molecules gradually surrounding ions

19
Q

The seperation of ions from each other

A

Dissociation

20
Q

The surrounding of solute particles by solvent

21
Q

How do you know a compound is electrolytic

A

If their aqueous solutions conduct electricity

22
Q

Why do molecular compounds not conduct electricity

A

becuase there isnt a presence of ionic bonds to conduct electricity

23
Q

What is the process of dissolving

A
  1. bonds between the particles in the solute break(endothermic)
  2. Intermolecular foces between particles in the solvent also break(endothermic)
  3. The attraction between the particles of a solute and the particles of solvent result in the formation of chemical bons(exothermic)
24
Q

What is an endothermic process

A

If more energy is absorbed to break the bonds then amount of energy releases when the bonds are formed, the change is endothermic.

25
What is an exothermic process
If more energy is released when the solute solvent bonds form than is required to dissolve the solvent then the overall process is exothermic
26
Solubility
Ability to dissolve
27
What is a saturated
Saturated is a state in which a solution contains the maximum amount of solute that can dissolve. After this point, any additional solute will not dissolve and will remain as a solid in the solution.
28
What is unsaturated
Unsaturated refers to a solution that has less solute than the maximum amount that can be dissolved. In this state, more solute can still dissolve without any of it remaining undissolved.
29
In what conditions are gases highly soluble at normally
at high pressures and low temperatures
30
In what condtions are solids highly soluble at normally
at high temperatures
31
In what conditions are liquids highly soluble at normally
at high temperature
32
solubility equilibrium
established by adding a solute to a solvent
33