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Science test (Chemistry) Flashcards

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1
Q

What is an isotope?

A

A form of the same atom that differ only in their number of neutrons

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2
Q

What is an electron?

A

A negatively charged particle within the atom

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3
Q

Atomic number

A

The number of protons an atom contains

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4
Q

What is the atomic mass?

A

The average mass of an atom
# of protons + # of neutrons
(sum of what is in the nucleus)

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5
Q

What are all of the diatomic molecules?
(Think: Have No Fear Of Ice Cold Beer)

A

Hydrogen
Nitrogen
Fluorine
Oxygen
Iodine
Chlorine
Bromine (Br)

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6
Q

How do you name a covalent bond from formula?

A
  1. Name first element, and add prefix if there is more than 1 atom of this element
  2. Name second element and add prefix and change the end to ide.
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7
Q

What is a chemical bond?

A

A chemical link between two or more atoms, holding the atoms together

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8
Q

Is the nucleus positively or negatively charged?

A

Positively charged

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9
Q

Periods. Horizontal or vertical?

A

Horizontal

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10
Q

Prefixes for 1 atoms, 2 atoms, 3 atoms, 4 atoms, 5 atoms:

A

1 = mono
2 = di
3 = tri
4 = tetra
5 = penta

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11
Q

What is an ion?

A

An atom lost or gained electrons.There are cations (positively charged), and anions (negatively charged)

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12
Q

What is a subatomic particle?

A

A particle that is smaller than an atom.These particles are found within an atom

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13
Q

What is an anion?

A

A negatively charged ion

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14
Q

Cation?

A

A positively charged ion

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15
Q

What is a molecule?

A

Two or more atoms chemically bonded together

Also known as the smallest discrete particle of a pure substance

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16
Q

What is a covalent bond?

A

A chemical bond that involves the sharing of electrons to form electron pairs between atoms.

Unlike an ionic bond, the electrons are not transferred from one atom to another. Instead, they are shared between the atoms.

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17
Q

Ionic bonds

A

A chemical bond between two oppositely charged ions; the metal becomes positively charged as it gives up electrons, and the non-metal becomes negatively charged as it gains electrons from the metal)

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18
Q
A
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19
Q

Chemical vs physical properties

A

Chemical properties can be observed or measured when a substance undergoes chemical change.
Physical properties do not need to undergo chemical change to be observed or measured.

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20
Q

Chemical vs physical change

A

Chemical change = chemical composition of substance changes or something new is created.
Physical change = substance change without anything new being created or without a change of chemical composition (Ex: a change in state of matter, or the substance being cut)

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21
Q

Qualitative vs quantitative physical properties

A

Quantitative physical properties = properties that can be measured or calculated

Qualitative physical properties = properties that are observed without measuring.

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22
Q

Ways to describe chemical properties (found during a chemical change):

A

Reactivity with other substances (with water, oxygen, and acid)

Combustibility (the ability of an element or compound to burn in the air)

Odour

Colour change

Precipitate(s)

Bubbles

Gas produced

Temperature change

Corrosion

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23
Q

Sublimation is when solid turns directly into a gas. How does this happen?

A

Sublimation occurs when the particles of the solid gain enough energy to lose the force of attraction between them.

Gain enough energy, lose force of attraction

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24
Q

Deposition is when

A

a gas turn directly into a solid

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25
Pure substance vs mixture
Pure substance = made up of one type of particle and cannot be separated by any physical means Mixture = a combination of different types of particles that retain their chemical identity
26
A pure substance can be an element or compound. What are they?
Element = one type of atom Compound = two or more types of atoms chemically bonded
27
A mixture can be a homogeneous mixture or a heterogeneous mixture. What are they?
Homogeneous = appears uniform without (solution, where particles are all combined) Heterogeneous (hetero is avg and on avg you can see components) = colloids (particles scattered evenly throughout) and suspensions (suspended particles will settle)
28
Create a graph showing the differences between metals and non metals and metalloids
GO!
29
Review the putting metals to work sheet (pg 66)
30
How does deposition occur?
For depostion to occur, thermal energy must be removed from a gas.
31
Selected property of chromium
Resists corrosion (good for chrome plating)
32
Selected property of copper and aluminum
Good conductor (good for electrical wiring)
33
Selected property of Nickel
Resists corrosion (good for coinage)
34
5 keys in particle theory:
1. All matter is made up of particles 2. All particle have space between them 3. Particles are always moving 4. Particles move faster and further apart when heated 5. All particles are attracted to eachother
35
In covalent bonds, what do you draw in Lewis dot to show bond between 2 electrons?
1 line instead of the 2 dots
36
How do you know if the is molecule an ionic or covalent compound?
Ionic is made of metals and non-metals Covalent is made up of non-metals only.
37
What does the staircase on the periodic table represent?
It shows where the metalloids are, and it is the transition between metals and non-metals
38
How do you name an ionic compund from formula?
1. Write the name of the first element 2. name second element and change the end to 'ide'.
39
Atomic # = ?
= # of protons
40
Mass # = ?
= # of protons + neutrons
41
When atom gains electrons, negative charge is formed. When atom loses electrons what charge is formed?
Positive charge
42
To find number charge of an ion what formula do you use?
of protons -total # of electrons
43
Example of deposition
Frost. The water vapor in the air lies on a surface that has a temperature below freezing, turning the water vapor into frost.
44
An example of sublimation
Dry ice. When the solid/frozen carbon dioxide gets exposed to air it changes directly into a gas
45
Isotope vs Ion
An isotope is a form of an atom with a different number of neutrons than protons. An ion is atom that has lost or gained electrons.
46
Why do atoms gain or lose electrons
To have full valence shells. Having full valence shells makes them more stable, which leads to them having more energy
47
Which elements gives away valence electrons?
Metals
48
Which groups take away electrons?
15 (nitrogen family), 16 (oxygen family), and 17 (halogens). The non-metals
49
Do happy campers ever become ions? Why?
Never. They have filled electron shells with no half-filled orbitals available for making covalent bonds
50
What are diatomic molecules?
Amolecule made up of only 2 of the same element (Ex: O2)
51
Phases are used in describing mixtures. What is a phase?
A distinctly uniform sample of matter is said to have one phase. (Ex: Coffee with cream and sugar)
52
Where are metals, metalloids, and non-metals located on the periodic table?
Metals: Left (majority) Metalloids: along the staircase Non-metals: right
53
What is a compound?
A substance made up of more than one type of element
54
Usual state of matter of metals:
Solids
55
Usual state of matter of non-metals:
Gases and powdery solids
56
Metal vs non-metals. Which has more lustre?
Metals
57
Metals vs non-metals. Which is more brittle?
Non-metals
58
Metals vs non-metals. Which are better conductors?
Metals
59
Metals vs non-metals. Which has a higher boiling and melting point?
Metals
60
Hydrogen is very explosive if not...
combined with other elements
61
What causes noble gases to glow?
An electrical current passing through them makes them glow
62
Metals include 2 groups we are focused on, which are:
Alkali metals Alkaline Earth metals
63
Non-metals include 2 groups we are focused on, which include:
Halogens Noble gases
64
Left to right of periodic table, atomic radius BLANK Top to bottom, atomic radius BLANK
Blank 1: Decreases Blank 2: Increases
65
Why does the atomic radius decrease from left to right of periodic table and increase from top to bottom?
When the atomic number gets higher, so does the number of protons. The more protons, the greater the amount of positive energy to attract the electrons (bring them in closer, decreasing the radius). It increases down a group, because the number of energy levels (n) increases, so there is a greater distance between the nucleus and the valence shell
66
Positive and negative ions attract each other, creating...
Ionic compounds
67
With the Lewis Dot Diagram, what do you include
Element symbol and number of valence electrons in form of a dot
68
What is a subscript?
The number is written in the lower right corner to represent more than one atom of the element, chemically combined.
69
Subscript at the end of a bracket...
Multiplies with all of the subscripts in the bracket
70
Coefficient indicates the number of atoms of an element or molecule
71
3C vs C3
C C C vs C3(chemically combined)
72
How do we know atoms exist?
- chemical reactions we can observe their effects - mathematic equations and indirect observations, we can calculate their various sizes - the aid of new tech such as the scanning tunnelling microscope, we can see them.
73
What is an inert gas?
Another way to say 'noble gas'
74
Characteristics of noble gases:
full valence shells very stable and very low chemical reactivity low melting and boiling points
75
Characteristics of alkali metals
very reactive 1 valence electron high conductivity
76
Characteristics of alkaline earth metals
reactive but not as reactive as the alkali metals 2 valence electrons good conductors
77
Characteristics of halogens
highly reactive 7 valence electrons toxic
78
What is the difference between a molecular element, a molecular compound, and an ionic compound?
Molecular element: a molecule that is made up of atoms of the same element. Could also be called a diatomic molecule Molecular compound: molecules comprised of atoms of different elements Ionic compound: a compound formed when oppositely charged ions of different elements attract each other.
79
How do particles overcome attraction?
When energy is added in the form of heat, the particles aquire enough energy to overcome the force of attraction between them.
80
What is the difference between atomic number, mass number and the atomic mass?
Mass number: The sum of the number of protons and the number of neutrons in an atom. Atomic number: The number of protons in an atom. Atomic mass: The average mass of an atom, taking into account all its naturally occurring isotopes

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