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CST Review Flashcards

To help students review concepts covered in Chemistry this year in preparation for the CST test.

1
Q

What is the name of a positively charged ion?

A

cation

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2
Q

What is a compound made from 2 nonmetals called?

A

molecule

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3
Q

What is the number in front of a substance in a balanced equation?

A

coefficient

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4
Q

How many electrons does carbon need to become full like a noble gas?

A

4

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5
Q

What period does magnesium belong to?

A

3

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6
Q

What is the name of elements that belong to group 7A?

A

Halogens

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7
Q

What group is stable and does not react in the natural world?

A

Noble gases, group 8A

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8
Q

What does the atomic number of an element identify?

A

the number of protons in the nucleus

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9
Q

What 2 subatomic particles contribute to the mass of an atom?

A

protons and neutrons

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10
Q

what step of the scientific method is an educated guess based on research?

A

Hypothesis

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11
Q

Where are the transition metals found on the periodic table?

A

middle, B group

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12
Q

What is the mass of a proton?

A

1 atomic mass unit (amu)

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13
Q

What is the molar mass of a substance?

A

The mass of a substance in grams ( 1 mole)

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14
Q

What do metals do with their valance electrons?

A

lose them to form cations

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15
Q

What is a negatively charged ion called?

A

anion

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16
Q

What type of bond holds a metal and a nonmetal together?

A

ionic

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17
Q

What is the mass of 44.8 L of oxygen gas (O2) at STP?

A

64 grams

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18
Q

What are the 7 diatomic elements?

A

Br2 I2 N2 Cl2 H2 O2 F2

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19
Q

What is a beta particle?

A

an electron 0 e

-1

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20
Q

What are gamma rays?

A

High energy rays that penetrate through everything except lead and concrete

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21
Q

If a molecule is made of only C and H, what type of bond must hold it together?

A

covalent

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22
Q

when atoms donate and accept electrons what type of bond is formed?

A

ionic

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23
Q

Where is most of an atom’s mass found?

A

In the nucleus

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24
Q

what is a valence electron?

A

the electrons found at the outermost energy level

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25
what element would end at 4s2 3d10 4p5?
Bromine Br
26
What is the standard molar volume?
22.4 Liters
27
How many particles are in a mole?
6.02 x 10 23
28
If one mole of glucose has a mass of 180 grams, how many grams would 0.5 moles weigh?
90 grams
29
How would you balance this equation? | C2H6 + O2 --> CO2 + H2O
2C2H6 + 7O2 --> 4CO2 + 6H2O
30
What is the equation for the ideal gas law?
PV = nRT
31
How do you convert 53oC to K?
53 + 273 = 326K
32
Random motion of a gas molecules produces what?
Pressure on a surface
33
How do you describe the relationship between P and V?
Inversely proportional
34
The periodic table is organized according to what?
atomic number ( # of protons)
35
Where are the metals on the periodic table?
on the left of the dividing line
36
Where are the nonmetals on the periodic table?
on the right of the dividing line
37
What is the name given the elements that display both metallic and nonmetallic properties?
semimetals or metalloids
38
How do you determine how many valence electrons an element has available to react?
group number (1A, 2A etc)
39
What element has the highest electronegativity?
Fluorine
40
What is the trend for atomic size (radius) going across a period?
size decreases as move from left to right due to effective nuclear charge
41
Describe the structure of an atom.
Nucleus has protons and neutrons, contains all the mass, mostly empty space, neutral ( P = e), electrons live in energy levels in the electron cloud and orbit around the nucleus
42
What are the building blocks of proteins?
amino acids
43
What type of bonds hold biological macromolecules together?
covalent
44
What are the 4 major biomolecule groups?
Proteins, lipids, carbohydrates, nucleic acids
45
How many dots would be drawn around a Fluorine atom and how would they be arranged?
7 electrons, 3 pairs and 1 single
46
What causes pressure?
collisions with the surface of a container
47
Why does Kelvin have to be used in gas laws problems?
Because we can reach OoC which cannot go in the bottom of a fraction
48
What are the values of standard temperature and pressure?
273 K and 1 atm (or 760 mmHg or 101.3 kPa)
49
Why do gas molecules diffuse through the air?
they move randomly and spread out to fill the container/room they are in
50
How do you know a compound is an acid?
It begins with H+ (Hydrogen ions)
51
How do you know a compound is a base?
It contains OH- (Hydroxide ions)
52
What are properties of acids?
pH lower than 7, taste sour, feel like water, corrosive with metals, turn litmus paper red, found in foods
53
What are the properties of a base?
slippery, taste bitter, found in cleaning products, do not react with metals, pH above 7, turns litmus paper blue
54
What s the name of a reaction that includes an acid and a base?
neutralization
55
What is the name of an acid that fully dissociates in water?
Strong acid
56
What is the range of the pH scale and where does water go?
0 (acid) to 14 ( base) water is 7, neutral H= = OH-
57
What are the 2 parts of a solution?
solute ( thing that dissolves) | solvent ( thing dissolved in)
58
What is the formula for Molarity?
M = moles of solute / Liters of solution
59
What type of reaction releases heat as a product?
exothermic
60
What type of reaction has a change in Heat that is positive (+)
endothermic
61
What 3 things affect the equilibrium of a reaction?
Pressure (gases only), concentration, temperature
62
What must all reactions reach before they move forward to make products?
Activation energy
63
How does a catalyst speed up a reaction?
lowers the activation energy
64
What force overcomes the electromagnetic repulsion between protons in the nucleus of an atom?
Nuclear force
65
What name is given to radioactive atoms?
isotopes
66
What is an alpha particle?
helium atom 4 | 2 He
67
What is fission?
nuclear reaction where 1 atom becomes 2 new atoms
68
What is fusion?
nuclear reaction where 2 smaller atoms join together to form 1 new different element
69
Matter is made of atoms that have positive centers of neutrons and protons surrounded by a cloud of negatively charged electrons. This statement is a________.
Theory (atomic theory)
70
What did Rutherford's experiment with gold foil and X-rays help discover about the atom?
atom has a dense positively charged nucleus, atoms are mostly empty space
71
Why is cobalt placed before Nickel on the periodic table of elements even though Co has a higher average atomic mass than Ni?
It is based on number of protons ( atomic number) Co has fewer protons.
72
Which element is capable of forming stable. extended chains of atoms through single, double or triple bonds with itself?
Carbon
73
The volume of 400 ml of chlorine gas at 400 mmHg is decreased to 200ml at constant temperature. What is the new gas pressure?
800 mmHg (inverse proportion, cut it in half, double other one)
74
At what temperature will all molecular motion stop?
0 K (-273 oC)
75
Why do water and oil not mix?
water is polar and oil is nonpolar
76
If the solubility of NaCl at 25oC is 36.2 g /100g H20, what mass of NaCl will dissolve in 50.0g of H2O?
18.1 g (cut everything in half)
77
Is melting ice an exothermic or endothermic process?
endothermic (ice has to get warmer to melt)
78
Is condensation an exothermic or endothermic process?
exothermic ( heat has to leave the gas to return to the liquid state)
79
Of 4 different lab solutions, one with a pH of 11, one with pH 7, one with pH 5, and one with a pH of 3, the solution with the highest acidity would be pH?
3
80
How many atoms are in 97.6 grams of Platinum (Pt)?
3.01 x 10 23

Chemistry (2 decks)

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