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Exploring Matter - Unit Test Flashcards

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1
Q

Pure substance

A

Pure Substance: A substance that is made up of only one type of particle (ex. H20, gold, oxygen, etc.)

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2
Q

Mixture

A

A substance that is made up of at least 2 different types of particles.

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3
Q

Element

A

A pure substance consisting of atoms which all have the same number of protons. An element cannot be broken down into a simpler chemical substance by any physical or chemical means

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4
Q

Compound

A

A pure substance composed of two or more different elements that are chemically joined up.

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5
Q

Homogeneous mixture

A

A mixture which has uniform composition and properties throughout it (EX. salt and water)

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6
Q

Heterogeneous mixture:

A

Made up of different substances that remain physically separated (EX. sand and water)

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7
Q

Physical property

A

A characteristic of a substance that can be determined without changing the composition of that substance.

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8
Q

Quantitative physical property

A

A property of a substance that is measured and has numerical value (EX. temperature, mass, height, etc.)

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9
Q

Qualitative physical property

A

A property of a substance that is not measured and does not have a numerical value (EX. colour, odour, and texture)

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10
Q

Chemical property

A

A property of a substance that describes its ability to undergo changes to its composition to produce one or more new substances (EX. combustibility, reacts with water, etc.)

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11
Q

Physical change

A

A change in which the composition of the substance remains unaltered and no new substances are produced.

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12
Q

Chemical change

A

A change in the starting substance or substances and the production of one or more new substances.

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13
Q

Precipitate

A

An insoluble solid that emerges from a liquid solution

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14
Q

Atom

A

The smallest unit of an element

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15
Q

Molecule

A

Two or more atoms of the same or different element that are chemically joined together in a unit.

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16
Q

Valence electrons

A

The electrons on the outer orbit of an atom

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17
Q

Proton

A

A positively charged particle in the atom’s nucleus

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18
Q

Electron

A

A negatively charged particle in an atom

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19
Q

Neutron

A

A neutral particle in the atom’s nucleus (no charge)

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20
Q

Matter

A

Physical substance in general. Occupies space and mass.

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21
Q

Atomic number

A

The number of protons in an atom’s nucleus

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22
Q

Mass number

A

The number of protons and neutrons in an atom’s nucleus

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23
Q

Isotope

A

An atom with the same number of protons but a different number of neutrons

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24
Q

Ion

A

A particle that has either a positive or negative charge

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25
Cation
A positively charged ion
26
Anion
A negatively charged ion
27
Covalent bond
A bond formed when two non-metal atoms share electrons
28
Molecular compound
A molecule that consists of two or more different elements
29
Diatomic molecule
Elements that bond together in pairs (The Magic Seven)
30
What is the particle theory
A way to describe the structure of matter and how it behaves
31
Explain the particle theory
1. All matter is made up of different kinds of particles 2. Different substances are made up of different kinds of particles 3. Particles are in constant random motion 4. The particles of a substance move faster as the temperature increases 5. Particles attract each other
32
What are the three states of matter?
Solid, liquid, and gas
33
Review all diagrams
Double tap the home button bro 😋
34
Examples of physical properties
Lustre, viscosity, hardness, ductility and color
35
Malleability
The ability of a solid to be hammered out or bent into different shapes
36
Ductility
You ability of a solid to be pulled into wires
37
Hardness
The measure of the resistance of a solid to be scratched or dented
38
State
The form that matter is in while at room temperature
39
Crystal form
Regular shaped matter that has flat sides and angles into which a substance solidifies
40
Solubility
The ability of a substance to dissolve in a solvent
41
Viscosity
The property of a liquid that prevents it from flowing
42
Color
That sensation produced when wave lengths of light strike through the retina of the eye
43
Texture
The sensation caused by touching a substance to determine its outer feel
44
Optical clarity
The property that allows the transmission of light to pass completely, partly or not at all
45
Taste
The property that triggers four different sense organs in the mouth
46
Lustre
The brightness or dullness of a substance
47
Other types of physical properties
Brittleness, electrical conductivity, density, and count
48
Formulas for density? GRASS method?
``` D= m/v M= d x v V= m/d ``` ``` Given Required Apply equation Solution Statement ```
49
Examples of physical changes
Cutting up carrots, crumpling up a piece of paper, ripping the paper up into tiny pieces, any changes state, making a paper airplane and dissolving sugar in your coffee
50
Examples of chemical properties
Combustibility, reacts with water, reacts with oxygen, it reacts with acid
51
Evidence of chemical changes
Change of color, bubbles are visible that are not caused by heating/boiling, heat or light given off, a solid or precipitate is formed, difficult to reverse, change in odour
52
Chemical families in the periodic table
``` Different groups: Alkali Metals -group 1 -charge:+ -far left hand column -shiny, silvery, soft -extremely reactive and are found in nature as compounds ``` Alkaline Earth Metals - group 2 - charge:+2 - 2nd column from the left - shiny, silvery, not as soft as alkali metals - very reactive, not found free in nature Halogens - group 17 - charge:-1 - 2nd column from the right - most reactive non-metals - only appear as compounds in nature, usually with alkali metals - often found in living things Noble gases - group 18 - no charge - first column from the right - colourless, odourless, tasteless - non-toxic except for radon - the "boring" gases... almost totally un-reactive - do not form compounds Rare earth metals - at the bottom - lanthanide series (atomic numbers 57-71) and actinide series (atomic numbers 89-103) - most are synthetic or man-made
53
How was the periodic table arranged when Mendeleev created it?
- created in 1869 by Dimitri Mendeleev - only 63 elements known at the time - arranged the elements by increasing mass - then grouped the elements with similar properties together - left blank spaces in his table and used them to predict the properties of elements that have not been discovered yet
54
Present day arrangement of the periodic table
1. Arranged based on physical and chemical properties of the element - Group=column - elements in the same group have similar properties 2. In order of increasing atomic mass (basically) 3. In order of the atomic number of the elements and based on the atomic structure - period=row 4. Read like a book-each line is read left to right, top line to bottom line
55
Patterns in the periodic table
Metals: - left side, central region of the periodic table - solid, shiny Non-metals: - right side of the periodic table - solid, liquid or gas - dull lustre (powdery) Metalloids: -located between the metals and non-metals along the staircase line
56
Period
- a row on the periodic table - each period has the same number of orbits - # of period is equal to the number of orbits
57
Group
- a column on the periodic table - each group has the same number of valence electrons - # of group or last number in group number is equal to the number of electrons in the outer orbit (valence electrons) exception helium
58
Chemical family
A column of elements on the periodic table with similar properties
59
How do you calculate the number of protons, electrons and neutrons?
Protons: Atomic number Neutrons: Mass number - atomic number Electrons: Atomic number (in normal state)
60
What are atoms made up of?
Protons, electrons and neutrons
61
Describe the particles in an atom.
Proton: positive 1 charge, large, located in the nucleus, 1amu Electron: negative 1 charge, very small, located outside the nucleus, 0amu Neutron: no charge, large, located in the nucleus, 1amu
62
The atomic mass
- measured in amu (atomic mass unit) - when rounded is referred to as mass number - mass number= # of protons and # of neutrons in the atom's nucleus
63
Why is atomic mass a decimal number?
It is weighted the average of the masses of all of the isotopes of that element
64
Bohr-Rutherford diagrams
Used to represent the atomic structure of a atom
65
What order do you place electrons when you are drawing Bohr-Rutherford?
Top, bottom, right, left
66
Ionic compounds
Formed by metal ions and nonmetal ions. Metals form cations and non-metals form anions. These have opposite charges and are, therefore, attracted to each other.
67
Prefix rules
- A prefix is used on the first element when there is more than one atom - A prefix is always used on the second element - The ending of the second element is changed to "ide"
68
The magic seven
HOFBrINCl

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