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HESI-A2 > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Why does chemical bonding happen?

A

They form to make atoms more stable; atoms are “stable” when the outer orbital is “full”.

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2
Q

Ionic Bonds

A

One atom wants to give away an electron and one wants to take that electron so both are stable. Due to now opposite charges the two atoms stick together.
-Ex: Na ( has 1 electron, is neg. ) +Cl ( has 7 electrons, is pos. ) = Na ( becomes + cation, no ele. so is stable ) + Cl ( becomes - anion, has 8 ele. so is stable ).

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3
Q

Covalent Bonds

A

Atoms share electrons to become stable. Strongest bond that is not an IMF!

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4
Q

Polar Covalent Bonds

A

When the atoms are sharing electrons and the atoms have different charges.

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5
Q

Single Bonds

A

Only one pair of electrons is shared between two or more atoms ( only 2 electrons are shared ).
-Ex: H-O-H ; dashes represent single bonds.

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6
Q

Double bonds

A

Two pair of electrons are being shared ( 4 electrons involved ).
-Ex: O2 equals O=O ; two lines represents double bond.

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7
Q

Salts

A

Are formed from the remaining ions that do not form H2O ( acids + bases = try to neutralize each other and form H2O ).

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8
Q

Acids

A

Compounds that produces excess H+ ions.

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9
Q

Bases

A

Compounds that produce excess OH- ions.

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10
Q

Acid-Base concentration ( how is the acid-base measured )

A

Can be measured by the pH scale.

-Ex: 0-14; 0-6 is acidic, 7 is neutral, and 8-14 is basic.

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11
Q

Hydrochloric acid ( HCL )

A

Abundant amount of hydrogen chloride in water. Found in gastric juices; when not in gastric juices it is highly corrosive.

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12
Q

Liquid Drug Forms

A

Packaged in prefilled containers of stalk bottles.
Administered w/ : cups, teaspoons, needles attache to tubing or syringes, needle-less syringes, drops in mouth/eyes/ears, NG tubes.

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13
Q

Aqueous

A

Supplied in H2O-based solution,

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14
Q

Elixir

A

Sweetened w/ alcohol.

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15
Q

Emulsion

A

Mixture of 2 liquids that normally do not mix ( oil & water ).

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16
Q

Fluid

A

All liquid medications.

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17
Q

Drops

A

Liquid drops.

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18
Q

Half-strength

A

Solution has been diluted 50%.

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19
Q

Mixture

A

Compound medication consisting of more than one liquid medication.

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20
Q

Solution

A

H2O based liquid medication.

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21
Q

Suspension

A

Solid particles in a liquid medication that must be shaken gently & thoroughly

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22
Q

Atoms

A

Basic building blocks.
Nucleus contains ( + charges ) protons and neutrally charged neutrons.
Electrons ( - charged ) are on the outside of the nucleus.
Electrically neutral : atoms are - when more electrons than protons; atoms are + when more protons than electrons.

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23
Q

Atomic number

A

Number of protons in the nucleus. ( Above element symbol )

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24
Q

Atomic Mass

A

Number of protons and neutrons combined; or average mass of atoms isotopes. ( Below element symbol ).

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25
Q

Orbitals

A
  • Each orbital holds 2 electrons. Also arranged in energy levels.
  • Number = orbital #; letter= sublevel identification.
    • Sublevels: S= 1 orbital ( 2 electrons ), P= 3 orbitals ( 6 elec. ), D= 5 orbitals ( 10 elec. ), F= 7 orbitals ( 14 elec. ).
  • Arrangement: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 7s, 5f, 6d, 7p.
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26
Q

Energy levels

A

Energy level closet to the nucleus holds 1 orbital ( so only 2 electrons ). All other energy levels have 4 orbitals ( so 8 electrons ).

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27
Q

Isotopes

A

Two atoms that have the same atomic number but different atomic masses ( so diff. # of neutrons ).

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28
Q

Radioactive Isotopes

A

Isotope atoms w/ an unstable nucleus that radiates particles.

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29
Q

Redox reactions

A

Electrons are transferred from one atom to another. OIL ( Oxidation Is Losing; becomes + ) - RIG (Reduction Is Gaining; becomes - ).
*see notes in red spiral for clearer understanding

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30
Q

Description of matter

A

Anything that has mass or takes up space.

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31
Q

Combustion chemical reaction

A

When O2 combines w/ another compound to form H2O and CO2.
Exothermic reaction-produces/needs heat.
( A+O2 —-> CO2+ H2O [uses heat] )

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32
Q

Synthesis chemical reaction

A

Two or more simple compounds/atoms combine to form a more complicated compound.
( A + B —-> AB ).

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33
Q

Decomposition chemical reaction

A

Breaking down a complex molecule into simpler compounds/atoms.
( AB —-> A + B ).

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34
Q

Single-replacement chemical reaction

A

When one cation/anion trades places w/ another in the compound.
( AX + B —-> BX + A ).

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35
Q

Double-replacement chemical reaction

A

When the cations or anions of two different molecules trades places; now forming 2 different compounds.
( AB + CD —-> AD + BC ).

36
Q

Acid-base neutralization chemical reaction

A

Special kind of double-replacement reaction that takes place when and acid and base react w/ each other to form H2O and salt.
( HX + BOH —-> BX + H2O ).
( acid + base —–> salt + water ).

37
Q

Viscosity

A

Behavior of the flow of fluids described by two properties:

  • Density of fluids
  • Newtons law-affected by temp. and pressure
38
Q

Gas Laws

A
  • Volume
  • Temperature
  • Pressure
  • Moles ( amount )
39
Q

VSPER: Non-polar

A

Charge distribution of electrons is symmetrical ( charges are the same ).

40
Q

VSPER: Polar

A

Charge distribution of electrons is asymmetrical ( not the same; different charges ).

41
Q

States of Matter

A
  • Solid
  • Liquid
  • Gas
  • Plasma
42
Q

IMF stand for?

A

Intermolecular Forces. Forces that are between molecules.

43
Q

IMF : Dipole-dipole interaction

A

Each molecule is polar ( opposite charges ).

44
Q

IMF : Hydrogen bonding

A

Positively charged hydrogen and electronegative element ( such as Florine, Oxygen, or Nitrogen [ FON] ). Type of dipole-dipole interaction. Is the strongest IMF force.

45
Q

IMF : London Dispersion forces

A

Weakest IMF. Low boiling point. Mostly gases. Both molecules are non-polar.

46
Q

Van Der Waals bonding

A

Weakest type of chemical bonding.

47
Q

Water

A

Solvent in which most other compounds or solutes are dissolved in; aqueous solution.

48
Q

Dehydration synthesis

A

Reactions where water is lost from the reactants.

49
Q

Hydrolysis

A

Water is introduced to the reactants to brake the bonds, causing the reactants to be broken into smaller molecules.

50
Q

Energy definition

A

The ability to do work ( movement of an object by some force ). Two types main : kinetic and potential.

51
Q

Kinetic energy

A

Energy of motion.

-ex : a moving car has kinetic energy.

52
Q

Potential energy

A

Energy that matter gains from its arrangement or position. Object has the ‘potential’ to do work.
-ex : a car sitting ( not moving yet ) @ the bottom of a hill facing up; the car has the potential to drive up the hill.

53
Q

Mechanical energy

A

The sum of kinetic and potential energy.

-ex : a car driving up a hill has both kinetic and potential energy.

54
Q

Freezing point, boiling point, & normal body temperature in Fahrenheit?

A
  • 32 degrees
  • 212 degrees
  • 98.6 degrees
55
Q

Freezing point, boiling point, & normal body temperature in Celsius?

A
  • 0 degrees
  • 100 degrees
  • 37 degrees
56
Q

Fahrenheit to Celsius formula

A

F = C x 9 divided by 5 + 32

57
Q

Celsius to Fahrenheit formula

A

C = ( F - 32 ) x 5 divided by 9

58
Q

Kelvin to Celsius formula

A

Celsius = Kelvin - 273.15

- can then take Celsius to Fahrenheit.

59
Q

Cation

A

Positively charged ion.

60
Q

Anion

A

Negatively charged ion.

61
Q

The rows in the Periodic Table are called what?

62
Q

The columns in the Periodic Table are called what?

A

Groups.

- think of noble gases.

63
Q

Group I A of the Periodic Table have a _____ charge?

A

+ 1 charge; 1 valence electron.

64
Q

Group II A of the Periodic Table have a _____ charge?

A

+ 2 charge; 2 valence electrons.

65
Q

Group III A of the Periodic Table have a _____ charge?

A

+ 3 charge; 3 valence electrons.

66
Q

Group IV A of the Periodic Table have a _____ charge?

A

+ 2 or + 4 charge; 4 valence electrons.

67
Q

Group V A of the Periodic Table have a _____ charge?

A
  • 3 charge, 5 valence electrons.
68
Q

Group VI A of the Periodic Table have a _____ charge?

A
  • 2 charge, 6 valence electrons.
69
Q

Group VII A of the Periodic Table have a _____ charge?

A
  • 1 charge, 7 valence electrons.
70
Q

Group VIII A of the Periodic Table have a _____ charge?

A 
No charge ( octet is complete ); 8 valence electrons.
  - Noble gases group.
71
Q

What 4 factors increase reaction rate?

A
  • Increase temperature.
  • Increase surface area.
  • Introduce catalyst.
  • Increase concentration.
72
Q

Which material has the smallest specific heat?

73
Q

Specific Heat

A

Is the amount of heat required to raise the temperature of 1 gram by 1 degree Celsius.

74
Q

What is the SI unit of energy?

A

Joule.

- required energy for a force of 1 newton to act over a distance of 1 meter.

75
Q

Which kind of radiation has no charge?

76
Q

Radiation types?

A
  • Gamma
  • Alpha
  • Beta
77
Q

Gamma radiation

A

No charge

  • sunlight, radio waves
  • can penetrate human body
78
Q

Alpha radiation

A

+ 2 charge

79
Q

Beta radiation

A
  • ( neg ) 1 charge

- harmful to human health.

80
Q

What is the mass, in grams, of 1.0 mole of oxygen gas?

A
    • 1 mole times 2 oxygen molecules ( oxygen mass is 16 ).
        • so 2 x 16 = 32.
81
Q

What is an Empirical Formula?

A

The smallest expression of a chemical formula; can not be reduced.

82
Q

CH is what type of formula?

A

Empirical Formula.

83
Q

What is another name for aqueous HI?

A

Hydriodic acid.

84
Q

What does polyatomic ion mean?

A

An ion composed of 2 or more elements.

85
Q

What element is not involved in many hydrogen bonds?

A

Carbon.

- Any element that is not FON ( Florine, Oxygen, or Nitrogen ).

HESI-A2 (2 decks)

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