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Chemistry Flashcards

(105 cards)

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0
Q

Give an example of a mechanical (homogeneous) mixture.

A

Muffin Breakfast cereal Wood

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1
Q

What are the 5 facts of the particle theory of matter?

A
  1. All matter is made up of particles that have large space between them 2. Different substances are made up of different 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
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2
Q

Give an example of a solution

A

Apple Juice Milk Salt Water

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3
Q

Give an example of an alloy

A

Steel Brass Solder

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4
Q

Give an example of covalent bonds

A

Water (H2O) Carbon Dioxide (CO2) Ammonia (NH3)

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5
Q

Give names of elements in the first 4 rows of the periodic table with symbol

A

Hydrogen (H) Helium (He) Lithium (Li) Beryllium (Be) Boron (B) Carbon (C) Nitrogen (N) Oxygen (O) Fluorine (F) Neon (Ne) Sodium (Na) Magnesium (Mg) Aluminum (Al) Silicon (Si) Phosphorus (P) Sulphur (S) Chlorine (Cl) Argon (Ar) Potassium (K) Calcium (Ca) Scandium (Sc) Titanium (Ti) Vanadium (V) Chromium (Cr) Manganese (Mn) Iron (Fe) Cobalt (Co) Nickel (Ni) Copper (Cu) Zinc (Zn) Gallium (Ga) Germanium (Ge) Arsenic (As) Selenium (Se) Bromine (Br) Krypton (Kr)

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6
Q

Give an example of Ionic Compound

A

Sodium Chloride (NaCl) Magnesium Oxide (MgO)

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7
Q

Pure substances can combine to form what?

A

Mixtures

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8
Q

Pure substances include what?

A

Elements and Compounds

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9
Q

Mixtures include what?

A

Mechanical Mixtures and Solutions

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10
Q

List different qualitative properties.

A

Lustre Optical Clarity Malleability Brittleness Viscosity Hardness Ductility Electrical conductivity Odour

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11
Q

Define Lustre and give an example if a high Lustre object and a low-lustre object.

A

Shininess or Dullness High Lustre - Silver Object Low Lustre - Rusty Nail

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12
Q

Define Ductility and give an example of a ductile object.

A

The ability for an object to be drawn (pulled) into finer strands Ductile - copper (can be turned into thin wires)

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13
Q

Define Electrical Conductivity and give an example of a good conductor and a poor conductor

A

The ability of a substance to allow electric current to pass through it Good conductor - Copper Poor conductor - Plastics

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14
Q

Define Optical Clarity.

A

The ability to allow light to flow through

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15
Q

Give descriptive words for the optical clarity with an example of each.

A

Transparent: Clear Blue Glass Translucent: Frosted Glass Opaque: Brick wall

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16
Q

Define Brittleness and give an example of a Brittle object and a non-Brittle object

A

Breakability or Flexibility Brittle object - Glass Non-Brittle object - Modelling Clay

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17
Q

Define Viscosity and give an example of a viscous and less viscous object

A

The ability of a substance to flow or pour readily Molasses - Viscous Water - Less Viscous

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18
Q

Define Hardness and give an example if an object that is high on the hardness scale and an object that is low on the hardness scale

A

The relative ability to scratch or be scratched by another object Diamond - High on the hardness scale Wax - Low on the hardness scale

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19
Q

Define malleability and give an example of a malleable and non-malleable object

A

The ability of a substance to be hammered into thin sheets or molded Silver - malleable Glass - non-malleable

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20
Q

Calculate the density of a metal sample that is 18.00 cm long and 9.21 wide, and 4.45 cm high and that has a mass of 14.25 kg. What is the identity of the metal.

A

G l = 18.00 cm w = 9.21 cm h = 4.45 cm m = 14.25kg m = 14250g R d = ?g/cm3 A d = m/v v = l * h * w S v = 18.00cm * 9.21 cm * 4.45 cm v = 738cm3 d = 14250g/738cm3 d = 19.3 g/cm S The density of the metal is 19.3 g. The metal is gold.

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21
Q

Define Physical change.

A

A change in composition of the material where no new substance is formed

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22
Q

Define Chemical Change and give examples of evidence of chemical change.

A

A change in substance and a new substance is formed Examples of chemical change: Colour change Odour change Precipitate production - a new solid is seen Energy change - a change in temperature or light

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23
Q

Define precipitate

A

A solid that separates from a solution

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24
Is a change in state of a liquid to a gas or a solid to a liquid a chemical or physical change?
Physical change
25
Alkali metals are in which row of the periodic table?
Row 1
26
Alkaline earth metals are in which row of the periodic table?
Row 2
27
Halogens are in which row of the periodic table?
Row 17
28
Noble-Gases are in which row of the periodic table?
Row 18
29
The most reactive metals are metals of which type? What do these metals react with? Why?
Alkali metals React with halogens because they have opposite charges and the Alkali metal is trying to get rid of an electron while the halogen is trying to gain an electron
30
What is the charge of Alkali metals?
1+
31
What is the charge of Alkaline Earth metals?
2+
32
What is the charge of halogens?
2-
33
What is the charge of noble gases?
Neutral
34
Metals are where on the periodic table?
Left side
35
Non-metals are where on the periodic table?
Right side
36
Name the transition metals in the first 4 rows of the periodic table and give their symbol.
Boron (b) Silicon (Si) Germanium (Ge) Arsenic (As)
37
Name the transition metals in rows 3 and 4 of the periodic table and give the symbol.
Aluminum (Al) Scandium (Sc) Titanium (Ti) Vanadium (V) Chromium (Cr) Manganese (Mg) Iron (Fe) Cobalt (Co) Nickel (Ni) Zinc (Zn) Gallium (Ga)
38
The most reactive gases are which type of gas? What do these gases react with? Why?
Halogens React with Alkali metals because they have opposite charges and the Halogen wants to gain an electron while the Alkali metal wants to get rid of an electron
39
What is the name of the bond that forms when metals from the left side of the periodic table interact with non-metals from the right side of the periodic table?
Ionic Bond
40
What is the name of the bond that forms between gases?
Covalent Bond
41
What do Bohr Rutherford diagrams (atomic diagrams) include?
Details of the nucleus (number of protons and neutrons) Electron arrangement
42
What does the atomic mass represent
Number of protons + number of neutrons
43
What revolves around the nucleus of an atom
Electrons (-)
44
What is an atom made of?
Electrons (-) Protons (+) Neutrons (neutral)
45
List different chemical properties
Explosive Flammable Corrosive Flammable Poisonous Reactive Biohazardous Toxic
46
Define a characteristic chemical property
A physical property that is unique to a substance an can be used to identify the substance
47
Define Density and give the density formula
A measure of how much mass is contained in a given unit of volume d=m/v
48
What is the difference between a qualitative and quantitative property
Qualitative properties are descriptive words to describe an object Qualitative objects are measurements and calculations such as the density of an object
49
When magnesium and oxygen react, is it a chemical change or physical change that takes place? What type of bond takes place?
Physical Change Ionic Bond
50
The freezing point of water is at what temperature? What is the boiling point of water? When water freezes into ice or turns into gas, is it a physical or chemical change that takes place?
Freezing point 0C Melting point 100C Physical change occurs when water freezes into ice or becomes a gas
51
Why does the water freeze at a lower temperature when there is salt in the water?
The salt interferes with the freezing process of the water
52
What element was used in the first light bulb? Why?
Tungsten was used because of it had a very high boiling point and the light was not going to burn.
53
How valence many electrons can there be in the first four shells?
First shell - 2 Second shell - 8 Third shell - 8 Fourth shell - 18
54
Why can water cause damage to other objects when it freezes?
Water becomes less dense and expands
55
Why does ice float on water?
Ice is less dense than water
56
What do Bohr diagrams (atomic diagrams) include?
Element symbols in the nucleus Electron arrangement
57
What do Lewis Dot diagrams (atomic diagram) include?
Valence electrons Element symbol
58
What two characteristics of atoms determine how it will make chemical compounds?
The number of valence electrons Atomic charge
59
Give an example of building materials (for making houses and other buildings) that is a pure element, a pure compound, an alloy (solid solution) and a mechanical heterogenous mixture
Pure element: Iron Pure compound: Glue Alloy (solid solution): Steel Mechanical (heterogenous) mixture: Wood
60
Explain How an Ionic bond works?
A Metal from one side of the periodic table bonds with a Gas from the other side. The metal gives its extra electrons to the Gas so the metal and Gas have complete shells. The metal will have a positive (+) charge while the gas will have a negative (-) charge. The opposite charges will attract.
61
Describe the electron transfer with Magnesium and Oxygen bonding. What type of bond is it? What are the charges of the 2 elements? What is the chemical formula of the newly formed compound?
Ionic bond. Magnesium gives 2 electrons to oxygen and gets a charge of 2. (Mg2+) Oxygen gains 2 electrons and gets a charge of -2. (O2-) MgO
62
How do molecular compounds (molecular elements) form?
Atoms share valence electrons.
63
Give an example of a molecular compound? List the molecular elements.
H2O (water) H2 O2 F2 Br2 I2 N2 Cl2
64
How many atoms of what elements in the molecule Al2(SO4)3? What is the name of the chemical compound?
Element name #of atoms Aluminum 2 Sulphur 3 Oxygen 12 Aluminum sulphate
65
What do the ending 'ate' stand for in a chemical compound?
Oxygen in chemical compounds that include metals
66
What does the prefix di stand for in a chemical compound?
2 atoms (a molecule) of a gas.
67
What does dioxide stand for?
2 Oxygen
68
What does electrolysis do?
Electrolysis separates covalent compounds into their original forms.
69
What can cause a chemical reaction? Why is there a chemical reaction in hydrogen peroxide (H2O2)
An imbalance of a substance can cause a chemical reaction There is an imbalance and the compound is trying to get rid of its extra Oxygen and starts a chemical reaction
70
What element is essential for burning?
Oxygen
71
What chemical compound can create an explosion?
Hydrogen and Oxygen H2O (water vapour)
72
What gas extinguishes fires?
Carbon Dioxide (CO2)
73
What is the main component of chalk and Limestone?
Calcium Carbonate
74
Draw a Bohr-Rutherford diagram for Sodium.
Sodium Bohr-Ruthorfurd Diagram ![]()
75
Draw a Magnesium Bohr Diagram.
Magnesium Bohr Diagram ![]()
76
Draw the chemical compound for C6H12O6 (Sugar) using the ball and stick diagram. ams.
C6H12O6 (Sugar) ![]()
77
Define Molecule.
Two or more atoms of the same or different elements that are chemically joined together in a unit.
78
Define Chemical Formula.
A notation that indicates the type and number of atoms in a pure substance.
79
Define Molecular Element.
A molecule consisting of atoms of the same element.
80
Define an Ion.
A particle that has either positive or negative charge.
81
Give the difference between a Cation and an Anion
A Cation is a positively charged ion. An Anion is a negatively charged ion.
82
Define an Ionic Compound.
A compound that consists of positively and negatively charged ions.
83
Define a Covalent Bond.
A bond formed when two non-metal atoms share electrons.
84
Define a Catalyst.
A substance that speeds up a chemical reaction but is not used up in a chemical reaction but is not used up in the reaction.
85
Define Element.
A pure substance that cannot be broken down into a simpler chemical substance by any physical or chemical means.
86
Define Element Symbol.
An abbreviation for a chemical element.
87
Define Chemical Compound..
A pure substance composed of two or more different elements that are chemically joined.
88
Define Metal.
An element that is lustrous, maleable, and ductile, and comducts heat and electricity.
89
Define Non-Metal.
An element, usually a gas or a dull powdery sold, that does not conduct heat or electricity.
90
Define Metalloid.
An element that has properties of bith metasls and non-metals.
91
Define Chemical Family.
A column of elements with similar properties on the periodic table.
92
Define Alkali Metal.
An element in Group 1 of the periodic table.
93
Define Alkaline Earth Metal.
An element in Group 2 of the periodic table.
94
Define a Noble Gas.
An element in group 18 of the periodic table.
95
Define a Halogen.
An element in group 17 of the periodic table.
96
Define a Period on the periodic table.
A row on the periodic table.
97
Define an Atom.
The smallest unit of an element.
98
Define an Electron.
A negatively charged partice in an atom.
99
Define a Proton.
A positively charged particle in an atom.
100
Define a Neutron.
A neutral particle in the atom's neucleus.
101
Define an atomic number.
The number of protons in the atom's neucleus.
102
Define the Mass Number of an atom.
The number of protons and neutrons in the atom's neucleus.
103
Define an Isotope.
An atom with the same number of protons but a different number of neutrons.
104
Define Atomic Mass.
The mass of an atom in atomic mass units (u)

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