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Science > Exploring Matter - Unit Test > Flashcards

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
Q

Cation

A

A positively charged ion

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26
Q

Anion

A

A negatively charged ion

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27
Q

Covalent bond

A

A bond formed when two non-metal atoms share electrons

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28
Q

Molecular compound

A

A molecule that consists of two or more different elements

29
Q

Diatomic molecule

A

Elements that bond together in pairs (The Magic Seven)

30
Q

What is the particle theory

A

A way to describe the structure of matter and how it behaves

31
Q

Explain the particle theory

A
  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
Q

What are the three states of matter?

A

Solid, liquid, and gas

33
Q

Review all diagrams

A

Double tap the home button bro 😋

34
Q

Examples of physical properties

A

Lustre, viscosity, hardness, ductility and color

35
Q

Malleability

A

The ability of a solid to be hammered out or bent into different shapes

36
Q

Ductility

A

You ability of a solid to be pulled into wires

37
Q

Hardness

A

The measure of the resistance of a solid to be scratched or dented

38
Q

State

A

The form that matter is in while at room temperature

39
Q

Crystal form

A

Regular shaped matter that has flat sides and angles into which a substance solidifies

40
Q

Solubility

A

The ability of a substance to dissolve in a solvent

41
Q

Viscosity

A

The property of a liquid that prevents it from flowing

42
Q

Color

A

That sensation produced when wave lengths of light strike through the retina of the eye

43
Q

Texture

A

The sensation caused by touching a substance to determine its outer feel

44
Q

Optical clarity

A

The property that allows the transmission of light to pass completely, partly or not at all

45
Q

Taste

A

The property that triggers four different sense organs in the mouth

46
Q

Lustre

A

The brightness or dullness of a substance

47
Q

Other types of physical properties

A

Brittleness, electrical conductivity, density, and count

48
Q

Formulas for density? GRASS method?

A 
D= m/v
M= d x v
V= m/d 
Given
Required 
Apply equation
Solution
Statement
49
Q

Examples of physical changes

A

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
Q

Examples of chemical properties

A

Combustibility, reacts with water, reacts with oxygen, it reacts with acid

51
Q

Evidence of chemical changes

A

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
Q

Chemical families in the periodic table

A 
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
Q

How was the periodic table arranged when Mendeleev created it?

A
  • 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
Q

Present day arrangement of the periodic table

A
  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
Q

Patterns in the periodic table

A

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
Q

Period

A
  • a row on the periodic table
  • each period has the same number of orbits
  • # of period is equal to the number of orbits
57
Q

Group

A
  • 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
Q

Chemical family

A

A column of elements on the periodic table with similar properties

59
Q

How do you calculate the number of protons, electrons and neutrons?

A

Protons: Atomic number
Neutrons: Mass number - atomic number
Electrons: Atomic number (in normal state)

60
Q

What are atoms made up of?

A

Protons, electrons and neutrons

61
Q

Describe the particles in an atom.

A

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
Q

The atomic mass

A
  • 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
Q

Why is atomic mass a decimal number?

A

It is weighted the average of the masses of all of the isotopes of that element

64
Q

Bohr-Rutherford diagrams

A

Used to represent the atomic structure of a atom

65
Q

What order do you place electrons when you are drawing Bohr-Rutherford?

A

Top, bottom, right, left

66
Q

Ionic compounds

A

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
Q

Prefix rules

A
  • 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
Q

The magic seven

A

HOFBrINCl

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