VOCABULARY OF CHEMISTRY
1. Substance
A type of matter with a fixed composition.
2. Element
If all the atoms in a substance has the same identity
it becomes {blank}.
3. Compound
A substance in which the atoms of 2 or more elements
are combined.
4. Heterogeneous
Mixture
Mixture in which different materials can easily be
distinguished.
5. Homogeneous
Mixture
Contains 2 or more gases, liquids, or solids
substances blended evenly.
6. Solution
Homogeneous mixture with particles so small that they
cannot be seen with a microscope.
7. Colloid
Type of mixture with particles that are larger than
those in solutions, but not heavy enough to settle out.
8. Tyndall
Effect
Scattering of light by colloidal particles.
9. Suspension
Heterogeneous mixture containing a liquid where
visible particles settle.
10. Physical
Property
Characteristic of a material you can observe without
changing the identity.
11. Distillation
A process for separating substances by evaporating a
liquid and recondensing its vapor.
12. Chemical
Property
Characteristic of a substance that indicates whether
it can undergo a chemical change.
13. Chemical
Change
A change of one substance to another.
14. Law of
Conservation and Mass
The mass of all substances that are present before a
chemical change equals the mass of all the substances after the change.
15. Kinetic
Theory
Explanation of how particles in matter behave.
16. Melting
Point
The point in temperature when the solid starts to
liquefy.
17. Heat of
Fusion
The energy required to change a substance from a solid
to a liquid at its melting point.
18. Acid
An acid is a
compound with a pH of less than 7 that forms hydrogen ions when dissolved in
water. Acids react when coming into contact with bases and some metals to form
salts.
19. Alkali
metals
The alkali metals are the elements in the first column
of the periodic table with the exception of hydrogen.
20. Protons
Particles in a atom with a positive charge.
21. Neutrons
Particles in a atom with no charge.
22. Electrons
Particles in a atom with a negative charge.
23. Quarks
Smaller particles in neutrons and protons.
24. Electron
Cloud
Area around a nucleus where electrons are mostly
found.
25. Atomic
Number
Number of protons in an atom is equal to a number
called {blank}.
26. Mass Number
This number is the sum of the number of protons and
neutrons.
27. Isotopes
Atoms of the same element that have different numbers
of neutrons.
28. .Metals
Good conductors of heat and electricity.
29. Metallic
Bonding
Positively charged metallic ions surrounded by a
electron cloud.
30. Transitional
Elements
Between groups 1 and 2, and 13 and 18.
31. Nonmetals
Usually gasses or brittle solids at room temperature.
32. Diatomic
Molecule
Consists of 2 atoms of the same element in a covalent
compound.
33. Sublimation
The process of a solid going directly into a vapor.
34. Metalloids
Has properties of both nonmetals and metals.
35. Empirical formula
The composition of a compound in terms of the
relative numbers and kinds of atoms in the simplest ratio.
36. Semiconductors
Elements that conduct under circumstances.
37. Chemical
Formula
A formula that shows what elements are in a compound
and what it will become.
38. Chemical
Bond
Force that holds atoms together in a compound.
39. Ionic Bond
Force of attraction between opposite charges.
40. Oxidation
Number
Tells you how many electrons an atom has gained or
lost.
Give examples of metals in everyday life?
BalasHapusIron, tin, aluminum, nickel, copper, silver, gold
Hapuscould you tell me about sublimation??
BalasHapusSublimation is a term in chemistry related to substance changes. In addition, the term sublimation is also used to refer to one method of separation of chemical mixtures. In the case of substance change, sublimation is the change of the substance from solid to gas or from gas to solid. When the constituent particles of a solid are given a temperature increase of a certain amount, then the particle will sublimate to a gas. Conversely, when the gas temperature is lowered, the gas will soon change its form to be solid again.
HapusThe process of separating the mixture sublimation is by heating solids dissolved in solids so that the solid we want to take will turn into gas. The resulting gas is accommodated, then cooled again. The condition of separation of the mixture by means of sublimation is that the mixed particles must have large boiling point difference so that we can produce high purity steam.
Sublimation Example
The easiest example of sublimation we see is in the process of making blurry. The mixture of camphor and charcoal is heated so that the sublimed camphor will evaporate. After that the substance is cooled to become solid again.
I want to ask why on an atomic number element is the same as proton. Please explain.
BalasHapusCan you give me some example about acid? By the way your article look so good ☺️
BalasHapus
Hapus1. hydrochloric acid = HCL
2.Slanid acid = HCN
3.Samida sulphide = H2S
4. sulfuric acid = H2SO4
5. Phosphite Acid = H3PO4
6.asam Arsenate = H3ASO4
7.asam benzoate = C6H5COOH
8. Boramic acid = H3BO3
9.asam carbonate = H2CO3
10.asam formiat = HCOOH
11. Acid iodide = HI
12.asam bromide = HBR
13. Flaosida Acid = HF
14.asam nitrate = HNO3
15. Nitrite Acid = HNO2
16. Phosphoric acid = H3PO4
17. flocyanic acid = H5CN
18. Acid asitat = CH3COOH
19.Sam formal = HCOOH
20.asam finol = C6H50H
please give me example of chemical property!!
BalasHapusChemical properties are a matter related to substances altering the composition to form other substances. Examples are flammability, reactivity and oxidation.
HapusFlammability is the ability of a substance to eradicate oxygen. Examples of combustible materials are ethanol. When ethanol and oxygen. Chemical reaction, it releases energy in the form of heat and light.
Ethanol + Oxygen -> Carbon Dioxide + Air + Fire
What is the effect of Brownian motion on the colloidal system? Explain!
BalasHapusBrownian motion
HapusBrownian motion is the movement of colloidal particles that always move straight but erratic (motion track / irregular). If we observe colloid under ultraviolet microscope, then we will see that the particle will move to form zigzag. This zigzag movement is called Brownian motion. Particular particles are always moving. The movements can be random as in liquids and gases (backward Brown), whereas in solids only beroszillasidi place (excluding Brownian motion).
For colloids with a liquid or gas dispersing medium, the movement of particles will result in collisions with the colloidal particles themselves. The collision took place from all directions. Because the particle size is small enough, the collisions that occur tend to be unbalanced. So there is a resultant collision that causes changes in the direction of motion of particles resulting in the motion of zigzag or Brownian motion. The smaller the size of colloidal particles, the faster Brown's motion takes place. Similarly, the larger the size of colloidal particles, the slower the Brownian motion occurs.
This explains why Brownian motion is difficult to observe in solution and is not found in the heterogeneous mixture of liquids with solids (suspension). Brownian motion is also affected by temperature. The higher the temperature of the colloidal system, the greater the kinetic energy the particles of the dispersing medium are. As a result, Brown's motion of the dispersed phase particles is accelerating. Similarly, the lower the temperature of the colloidal system, the slower the Brownian motion.
could you explain to me about Tyndall Effect?
BalasHapus
HapusTyndall Effect
Tyndall effect is a symptom of scattering light rays (light) by colloidal particles. This is because the size of the colloidal molecule is quite large. This Tyndall effect was discovered by John Tyndall (1820-1893), a British physicist. It is therefore called the Tyndall effect.
The Tyndall effect is the effect that occurs when the solution is exposed to light. If the solution is actually irradiated with light, the solution will not enlarge the light, whereas in the colloidal system light will disappear. This happens because the colloidal particles have particles large enough to spread them. In contrast, in the actual solution, the particles are relatively small so scattering occurs only slightly and is very difficult to observe.