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CHM 1230 > quiz 1 > Flashcards

quiz 1 Flashcards

1
Q

what are the two characteristics of measurements that scientists are concerned with?

A

accuracy and precision

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2
Q

accuracy

A

how correct the measurement is. When measuring something, it is always desirable to get the “right” answer!

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3
Q

precision

A

how close a set of measurements of the same thing are to each other.

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4
Q

density

A

the ratio of a substance’s mass to its volume. It can be expressed by the equation d = m / v
(mass / volume)

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5
Q

finding mass of a solid

A

the amount of material in the sample.

- Many solids can be placed directly on the pan of a balance to determine their mass

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6
Q

finding mass of a liquid

A

the liquid must be placed in a pre-weighed container, and the container must then be re-weighed with the liquid in it
(finding mass by difference)

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7
Q

volume

A

the amount of space a sample occupies.

  • If the sample is a liquid, its volume can be measured directly by placing it in a calibrated container
  • read the meniscus
  • If the sample is a rectangular solid, its volume can be found by measuring the length, width, and height of the object, and multiplying the three together: V = L × W × H.
  • If the solid has an irregular shape, we can find its volume by immersing it in a known amount of liquid, and determining the volume of liquid displaced by the solid. (finding the volume by displacement) V2 - V1
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8
Q

meniscus

A

the low point in the lens-shaped surface of the liquid in a cylinder

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9
Q

Ammonia (NH3)

A

a waste product, forms by protein digestion and from intestinal bacteria.

  • Ammonia can build up in the blood if there are kidney problems, Reye’s syndrome, liver disease, and some genetic diseases.
  • Ammonia can cross the blood–brain barrier, leading to mental and neurological changes that may result in death.
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10
Q

Calcium ion (Ca2+)

A

needed for bones and teeth; it is also necessary for muscle contraction.
- High or low calcium levels can be present in diseases of the thyroid and parathyroid glands

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11
Q

Carbon dioxide (CO2) and hydrogen carbonate ion (HCO3 -1)

A

present in the body to help maintain the acid–base level, or pH, of your body.
- pH imbalances can be caused by electrolyte imbalance, kidney disease, hypertension, and the use of some medications

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12
Q

Chloride ion (Cl -1)

A

present in blood and in extracellular fluid.

  • It helps to maintain the body’s pH and regulates fluid levels.
  • Imbalances can result from dehydration or from acidosis (body pH decreases) or alkalosis (body pH rises).
  • Changes in chloride often mirror those of sodium.
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13
Q

Copper ion(II) (Cu2+)

A
  • plays an important role in enzymes that help regulate iron metabolism, form connective tissue, and produce energy.
  • Wilson’s disease, an inherited disease associated with excess storage of copper, causes liver and neurological damage.
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14
Q

Iron(II) ion (Fe2+)

A

needed to form red blood cells.

  • It is also a critical part of hemoglobin, the protein that carries oxygen throughout the body.
  • Low levels lead to anemia, while high levels can damage the heart, liver, and pancreas
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15
Q

Phosphate ion (PO4 3-) and related phosphorus-containing ions

A

bind with calcium and magnesium to strengthen bones and teeth, and helps to regulate the body’s pH.
- imbalances may signal kidney or gastrointestinal problems

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16
Q

Sodium ion (Na1+)

A

present in the body to help maintain proper fluid balance.

- Imbalances can be due to dehydration, fluid retention, and heart or kidney problems.

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17
Q

five types of chemical reactions that are commonly used to describe many of the chemical changes that occur around us every day

A
  1. Combination or synthesis reactions
  2. Decomposition reactions
  3. Single replacement reactions
  4. Double replacement reaction
    - two types of double replacement reactions:
    a. Precipitation reactions
    b. Neutralization reactions
  5. Combustion reactions
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18
Q

Combination or synthesis reactions

A

two elements or compounds combine to form one compound.

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19
Q

Decomposition reactions

A

one compound breaks up into two or more elements or compounds.

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20
Q

Single replacement reactions

A

where an element and a compound form a different element and different compound.

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21
Q

Double replacement reactions

A

where two compounds make two different compounds. There are two types of double replacement reactions:

a. Precipitation reactions
b. Neutralization reactions

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22
Q

DR: Precipitation reactions

A

where two compounds form two different compounds, where at least one of the products is a solid.

23
Q

DR: Neutralization reactions

A

where an acid and a base form water and a salt (anion + cation).

24
Q

Combustion reactions

A

where a hydrogen-and-carbon-and-maybe-oxygen- containing compound burns in oxygen to form carbon dioxide and water.

25
Q

Chemical reactions can be distinguished from physical changes at the macroscopic level if one of the following four observations are noted:

A

a gas is produced, a pre- cipitate (solid) forms, a color change occurs and a new color is observed, and a temperature change occurs.

26
Q

four common gasses

A

Hydrogen, oxygen, and carbon dioxide, and ammonia

27
Q

ammonia

A
  • It can often be identified by its smell, which may remind people of a beauty salon—perms and hair color often contain ammonia or ammonium compounds.
  • Ammonia can more safely be detected by wetting a piece of red litmus paper and holding it over the solid or solution that may contain ammonia.
  • The ammonia reacts to turn the litmus blue; the water simply makes the color change more obvious.
28
Q

when is hydrogen present?

A

Hydrogen is present if the flame extinguishes, frequently with a very faint whistling sound

29
Q

when is carbon dioxide present?

A

Carbon dioxide will extinguish the flame with no sound.

30
Q

when is oxygen present?

A

Oxygen’s presence will make the flame flare up and burn brighter.

31
Q

Carbonate compounds usually decompose to give

A

carbon dioxide

32
Q

hydroxide compounds often produce

A

hydrogen gas.

33
Q

solubility rules: soluble

A

Soluble Compounds (dissolve in water):

  1. Sodium, potassium, and ammonium compounds
  2. Acetates and nitrates
  3. Chlorides, bromides, iodides (halides); exceptions: Lead(II), mercury(I), and silver halides
  4. Sulfates; exceptions: Calcium, strontium, barium, and lead(II)
34
Q

solubility rules: insoluble

A
  1. Carbonates, chromates, and phosphates; exceptions: Sodium, potassium, and ammonium
  2. Hydroxide; exceptions: Sodium, potassium, and barium
  3. sulfides; exceptions: Sodium, potassium, ammonium, and calcium
35
Q

An ion

A

a chemical species that carries an electrical charge.

  • Neutral atoms get charged by either gaining or losing electrons.
  • If a neutral atom gains an extra electron it will become negatively charged (anions)
  • loss of an electron will cause the neutral atom to become positively charged (cations).
36
Q

common cations and anions

A 
calcium ion = Ca2+
barium ion = Ba2+
chloride ion = Cl-
sulfide ion = S2-
sodium ion = Na+
copper(II) ion = Cu2+
bromide ion = Br-
oxide ion = O2-
37
Q

Ionic compounds

A

made up of two separate and somewhat independent chemical species, a cation and an anion.

  • The cation is usually a metal ion
  • anion is almost always a nonmetal.
  • CaCl2 dissolved in water gives Ca2+ + Cl- + Cl-
  • In a compound, the sum of the positive charges must be balanced by the sum of the negative charges.
38
Q

testing for cations

A

In this experiment, you will be given photos of the flame test results for six different cations: Li+, Na+, K+, Ca2+, Sr2+, Ba2+
- You will also test for the cations by reacting them with three different reagents and
observing which cations will form a precipitate with the reagents:
Strontium ion + ammonium carbonate → cloudy white solution (a precipitate)
Lithium ion + ammonium carbonate → clear solution (no precipitate)

39
Q

There are only three anions you can have in your compound in today’s experiment and they are…

A

they are all halides (Cl–, Br–, and I–)

40
Q

Consider that both lithium and strontium give a red color in the flame test. If you have an unknown that gives a red color, how do you determine which metal ion is in the unknown?

A

Well, from the data above you would test your unknown by reacting it with ammonium carbonate. If no precipitate results it must be lithium, while a precipitate would indicate the presence of strontium.

41
Q

the halide test

A
  • When you do the halide test you will form the halogen in an aqueous (water based) solution.
  • Water is a polar solvent
  • The halogens you will be forming are nonpolar, so they are not very soluble in water, but you will be able to distinguish a difference in the color of the solution when the halogens are formed.
42
Q

halide test process

A

2 Cl– chloride ions colorless -> bleach -> Cl2
chlorine faint yellow
2 Br– bromide ions colorless -> bleach -> Br2
bromine orange/brown
2 I- iodide ions colorless -> bleach -> I2
iodine
purple/dark purple/black

43
Q

RAMP model

A

Recognize the hazard
Assess the risks of the hazard
Minimize the risks of the hazards
Prepare for emergencies caused by uncontrolled hazards

44
Q

corrosion

A

corrosion

  • skin corrosive/burns
  • eye damage
  • corrosive to metals
45
Q

exclamation mark

A
  • irritant
  • skin sensitizer
  • acute toxicity
  • narcotic effects
  • respiratory tract irritant
  • hazardous to ozone layer (non-mandatory)
46
Q

exploding bomb

A
  • explosives
  • self-reactive
  • organic peroxides
47
Q

skulls and crossbones

A

acute toxicity (fatal or toxic)

48
Q

flame

A
  • flammables
  • pyrophobics
  • self heating
  • emits flammable gas
  • self-reactives
  • organic peroxides
49
Q

gas cylinder

A
  • gases under pressure
50
Q

environment

A

aquatic toxicity

51
Q

health hazards

A
  • carcinogen
  • mutagenicity
  • reproductive toxicity
  • respiratory sensitizer
  • target organ toxicity
  • aspiration toxicity
52
Q

flame over circle

A

oxidizers

53
Q

density

A

mass / volume

CHM 1230 (1 decks)

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