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Chem Unit Flashcards

1
Q

What are the special groups/families found of the periodic table?

A
  1. Alkali metals
  2. Alkaline-earth metals
  3. Halogens
  4. Noble Gases
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2
Q

What is a common feature of the Alkali metals and where are they found on the periodic table?

A
  • Group 1

- React with H2O & Hallogens

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3
Q

What is a common feature of the Alkaline-earth metals and where are they found on the periodic table?

A
  • Group 2

- React with H2O

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4
Q

What is a common feature of Halogens and where are they found on the periodic table?

A
  • Group 17
  • React with Alkali metals
  • Have 7 valence electrons
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5
Q

What is a common feature of the Noble gases and where are they found on the periodic table?

A
  • Group 18

- Unreactive

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6
Q

What does the atomic number mean for atoms?

A

Atomic number = # of p+

Atomic number = # of e-

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7
Q

When an ion has a negative charge it ____________.

A

Gains electrons

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8
Q

When an ion has a positive charge it _____________.

A

Loses electrons

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9
Q

What is a Bohr diagram for an atom?

A
  • Consists of a nucleus (holds protons and neutrons), electrons, and electron shells
  • Up to 4 electron shells
    • Shell 1: 2 electrons
    • Shell 2: 8 electrons
    • Shell 3: 8 electrons
    • Shell 4: 18 electrons
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10
Q

What is a Bohr diagram for an ion?

A

Same as atom but with brackets around the diagram, stating the charge.

EX. (diagram)2-

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11
Q

What might an ion do to become “happy/stable”?

A

May lose shells/rings

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12
Q

What is an energy level diagram?

A

Consists of up to 5 different levels; 18e-
- Level 5: # of electrons (like 4th electron shell) ___________
- Level 4: # of electrons (like 3rd electron shell) 8e-
- Level 3: # of electrons (like 2nd electron shell) ___________
- Level 2: # of electrons (like 1st electron shell) 8e-
- Level 1: # of protons in nucleus ___________
2e-
___________
36p+

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13
Q

What is an Isotope?

A

An atom with different numbers of neutrons (which changes the mass #)

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14
Q

How is an isotope written?

A

Atom name - Mass # (ex. Sulfur - 33)

                   OR
         Mass #     \         /
                            \     /
                              \ /
                              / \
                            /     \
         Atomic #  /         \
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15
Q

How do you find the number of neutrons in an isotope? (n)

A

Subtract the Atomic # from the Mass #

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16
Q

How do you find the number of protons in an isotope? (p+)

A

Same as the Atomic #

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17
Q

How do you find the number of electrons in an isotope? (e-)

A

Same as the Atomic #

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18
Q

What is an atom and what is it’s characteristics?

A
  • The smallest fraction of an element that can exist
  • Composed essentially of electrons (1 negative charge), protons (1 positive charge), and neutrons (no charge)
  • Electrically neutral
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19
Q

What is an Ion?

A
  • An atom that is electrically charged, negative or positive (ex. Sulfur 2-)
       Positive ion-                                  Negative ion-
 Loses electrons                            Gains electrons
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20
Q

What is the lightest part of an atom?

A

The electron

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21
Q

What does the placement of an element on the periodic table tell us?

A

Period (rows) - Signifies the total number of electron shells in an element’s atom (Bohr)

Group (columns) - Represents the number of valence electrons of an element’s atom

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22
Q

What ion does an acid release in water?

A

H+ (hydrogen)

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23
Q

What ion does a base release in water?

A

OH- (hydroxide)

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24
Q

What colour does litmus paper change into?

A

Acid - turns/stays red
Base - turns/stays blue
Neutral - no change

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25
What elements are present in an Ionic compound?
Metals & non-metals
26
What elements are present in a molecular compound?
Non-metals
27
What is the state of an ionic compound at room temp.?
Solid
28
What is the state of an molecular compound at room temp.?
Solid, liquid or gas
29
Are molecular compounds conductive in water?
No.
30
Are ionic compounds conductive in water?
Yes.
31
What would an acid taste like?
Sour.
32
What would a base taste like?
Bitter.
33
What are the common solid molecular compounds to know?
Sugar (C6 H12 O6) and wax (C25 H52)
34
What are the common gas molecular compounds to know?
``` Carbon dioxide (CO2), Oxygen (O2), Carbon monoxide (CO), Carbon tetrahydride (CO4), Ammonia (NH3), Ethane (C2 H6) ```
35
How should you find the state of a ionic compound?
- Solubility table (look at 2nd element and match with 1st element. Very soluble= (aq) Slightly soluble = (s) PRECIPITATE) - Room temp = solid (s) - Molten = liquid (l) - Dissolved in water = (aq) - Aqueous = (aq)
36
What are the common liquid molecular compounds to know?
Br (l) and H2O (l)
37
How should you find the state of a molecular compound?
- Know from experience | - State will be indicated
38
What needs to be added to a compound's formula?
A subscript of the state; (ex. (s), (l), (g)
39
What prefixes should be used for a molecular compound with 7 atoms first and 9 atoms second?
Septa_____ nona_____ide
40
What prefixes should be used for a molecular compound with 6 atoms first and 5 atoms second?
Hexa______ penta________ide
41
What prefixes should be used for a molecular compound with 4 atoms first and 1 atom second?
Tetra______ mono______ide
42
What prefixes should be used for a molecular compound with 1 atom first and 10 atoms second?
_________ deca_______ide
43
What prefixes should be used for a molecular compound with 8 atoms first and 3 atoms second?
Octa______ tri______ide
44
What does it mean to have a diatomic atom?
When alone, they always have a 2 in after (O2)
45
What are the diatomic atoms?
``` Diatomic 7 (creates a 7 shape on the periodic table + hydrogen): H (hydrogen), N (nitrogen), O (oxygen), F (Florine), Cl (Chlorine), Br (Bromine), and I (Iodine). ```
46
Common molecular compounds to memorize: | What is the chemical formula of water?
H2O (l)(g)
47
Common molecular compounds to memorize: | What is the chemical formula of ammonia?
NH3 (g)
48
Common molecular compounds to memorize: | What is the chemical formula of methane?
CH4 (g)
49
Common molecular compounds to memorize: | What is the chemical formula of sucrose (table sugar)?
C12 H22 O11 (s)
50
Common molecular compounds to memorize: | What is the chemical formula of glucose?
C6 H12 O6 (s)
51
Common molecular compounds to memorize: | What is the chemical formula of Ozone?
O3 (g)
52
Common molecular compounds to memorize: | What is the chemical formula of sodium chloride (table salt)?
NaCl (s)
53
Common molecular compounds to memorize: | What is the chemical formula of ethanol?
C2 H5 OH (g)
54
Common molecular compounds to memorize: | What is the chemical formula of ammonium?
NH4 (s) * CANNOT be alone; unlike NH3 * Acts as a metal
55
Common molecular compounds to memorize: | What is the chemical formula of hydrogen peroxide?
H2 O2 (l)
56
What is the quick way to figure out if a compound is molecular or ionic?
Does it have a metal? Yes - ionic No - molecular (exception = NH4; acts like a metal)
57
What is the evidence of a chemical reaction?
Bubbles (proof of gas), energy change, odor creation, formation of a solid, colour change, pH change, oxidization, and/or flammability.
58
What is the meaning of endothermic
Absorbing energy, breaking bonds, cold
59
What is the meaning of exothermic?
Releasing energy, forming bonds, warm
60
What reaction type is this...? | 2 reactants = 1 product (reactant + reactant = product)
Formation/Synthesis- Two elements or compounds that combine to create a SINGLE product A + B = AB
61
What reaction type is this...? | 1 reactant = 2 products (reactant = product + product)
Decomposition - Reverse of formation Breakdown into it's elements AB = A + B
62
What reaction type is this...? | 1 reactant
Decomposition - AB = A + B
63
What reaction type is this...? | Creates CO2 & H2O
Combustion- | Burning of a hydrocarbon
64
What reaction type is this...? | Burning of a hydrocarbon (CxHy)
Combustion- | Creates CO2 and H2O
65
What reaction type is this...? | Compound + element = different compound + different element
Single Replacement- 1 swap Cations can only swap with cations Anions can only swap with anions AB + C = AC + B
66
What reaction type is this...? | 1 swap
Single Replacement- Compound + element = different compound + different element Cations can only swap with cations Anions can only swap with anions AB + C = AC + B
67
What reaction type is this...? | 2 swap
Double replacement- Cations can only swap with cations Anions can only swap with anions AB + CD = AD + CB
68
How do you name an ionic compound?
1. Write symbol of metal (consider it's charge) 2. Write symbol of non-metal (consider it's charge) 3. Balance charges to be equal (net zero) 4. Write number of atoms needed as a subscript 5. Write state as subscript i) Usually solid at room temp ii) Molten = liquid iii) Dissolved in water = aqueous iv) Solubility table
69
How do you name a molecular compound?
1. Write name of first element with appropriate prefix 2. Write name of second element with appropriate prefix 3. Change suffix of second element to "ide"
70
How do you name a base?
Same as an ionic compound - 1. Write symbol of metal (consider it's charge) 2. Write symbol of non-metal (consider it's charge) 3. Balance charges to be equal (net zero) 4. Write number of atoms needed as a subscript 5. Write state as subscript (aq)
71
Why can you balance a chemical equation?
Antonie Lavoisier's Law of Conservation of Matter- - Matter cannot be created or destroyed - Matter cannot be changed or rearranged - Mass of reactants = mass of products
72
How to balance a chemical equation?
1. Set up the reactant and (possibly predict) product | 2. Change coefficients to make the # of atoms/ charges equal on both sides
73
What are the polyatomic atoms?
O3 (ozone), P4, S8
74
What are the monatomic atoms?
Noble gases, all metals, carbon
75
What must be used when naming a molecular compound?
Prefixes according to the number of atoms
76
What are the attributes of an acid?
- Starts with H (hydrogen) EXEPTION: CH3COOH - Highly soluble (aq) - Conductive - Reacts with metals (bubbles; gas) - pH < 7
77
What should be added when writing an acid containing sulfur?
replace suffix with "ur" Examples: hydrogen sulfate - sulfuric acid hydrogen sulfite - sulfurous acid
78
What should be added when writing an acid containing phosphate?
replace suffix with "or" Examples: hydrogen phosphate - phosphoric acid hydrogen phosphide - hydrophosphoric acid
79
What are the attributes of a base?
- Ends with OH (hydoxide) - highly soluble (aq) - Does NOT react with metals - pH > 7 - Slippery feeling
80
How to predict products of chemical equations
1. Write the formulas for the reactants WITH states 2. Classify reaction type (Formation, Decomp, SR, DR, or combustion) 3. Predict the product(s) based on reaction type 4. Write the state of predicted product(s) 5. Balance like normal
81
What is Molar Mass?
The mass of 1 mol of any pure substance
82
How do you calculate the Molar Mass of a compound?
(Atomic mass of atom #1)(# of atoms) + (Atomic mass of atom #2)(# of atoms) = Molar Mass
83
What is a pair of electrons called?
A lone pair
84
What is a single electron called?
A bonding electron
85
What is the octet rule?
States that atoms bond to have 8 electrons in their outer-shell (like noble gas) EXCEPTIONS: Hydrogen (H) - needs 2 electrons on outer-shell Beryllium (Be) - needs 6 electrons on outer-shell
86
How should you know the state of an element?
Directly from the periodic table
87
What is an ionic hydrate?
An ionic compound containing H2O EX. CuSO4 + 5H2O ----------> Copper (II) sulfate pentahydrate
88
What is pH?
Potential Hydrogen Range 0-14 (most acidic - most basic) Difference between each number = 10x (pH of 3 is 10 times more acidic than pH of 4)
89
What are significant digits?
A way to write answers with proper accuracy
90
Are number 1-9 sig digs?
Yes
91
Are leading zeros (0.000003) sig digs?
No
92
Are trailing zeros (3.0089000) sig digs?
Yes
93
How many particles are in a mole?
602 000 000 000 000 000 000 000 | 6.02 x 10^23
94
When you are looking for the number of particles in more than one mole of a compound, what do you do?
Multiply the entire equation of (6.02 x 10^23) by the number of moles EX. 3 Moles - (3)(6.02 x 10^23) ---------> (18.06 x 30^69)
95
What was John Dalton's atomic theory?
Solid sphere - | The atom is the smallest particle of matter. It cannot be created or destroyed
96
What was JJ Thompson's atomic theory?
Raisin bun/Plum pudding - | Large (+) with small (-) embedded
97
What was Ernest Rutherford's atomic theory?
Nuclear model - | (+) nucleus that has p+ and all mass. e- move around the nucleus
98
What was Neil Bohr's atomic theory?
Electron shells/levels - | e- have fixed energy and move in circular paths around the nucleus which contains p+ and n

Science 10 (3 decks)

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