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CIH > IH Chemistry > Flashcards

IH Chemistry Flashcards

1
Q

Matter

A

Any that occupies space and has mass

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2
Q

Substance

A

Matter that has the same properties and composition e.g. atoms and molecules

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3
Q

Elements

A

A substance that cannot be decomposed to other substances

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4
Q

Compounds

A

Substance that consists of at least 2 elements and can decompose to other substances

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5
Q

Mixtures

A

Like compounds but components are interdependent and can be removed from the mixture

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6
Q

Atomic structure

A

Dense nucleus of protons and neutrons with outer volume containing electrons

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7
Q

Groups

A

Columns in periodic table, consists of elements with similar properties

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8
Q

Electron configuration

A

Electron filling scheme for a given element

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9
Q

Chemical properties

A

Bonding characteristics of an element though valence electrons. Similar properties should have similar valence shell configurations.

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10
Q

Covalent bonding

A

Atoms share electrons

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11
Q

Ionic bonding

A

Transfer of electrons

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12
Q

Octet rule

A

The tendency for an atom to have 8 valence electrons

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13
Q

Polar covalent bond

A

Uneven electron density in a covalently bonded molecule

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14
Q

Electronegativity

A

The tendency for an atom to have higher electron density

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15
Q

What molecules tend to be nonpolar?

A

Ax and CxAy

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16
Q

What is the Law of Conservation of Energy?

A

Energy cannot be created or destroyed, only change in form

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17
Q

Heat of reaction

A

The energy released or absorbed in a reaction

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18
Q

Solid

A

Definite shape and volume, strong intermolecular forces

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19
Q

Crystalline solid

A

Solid with crystal structure

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20
Q

Amorphous solid

A

Solid without a crystalline structure

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21
Q

Liquids

A

Molecules held a relatively small distances within a definite volume at a fixed temperature

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22
Q

Gases

A

Weak intermolecular forces, fills the shape of the container. Volumes affected by temperature and pressure.

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23
Q

Aliphatic hydrocarbon

A

Saturated, single bonds, non-polar

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24
Q

Unsaturated hydrocarbon

A

Double or triple bonds (alkenes, alkynes)

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25
Q

Aromatic hydrocarbons

A

Ring structure, follows Huckel’s rules

26
Q

Methyl

A

1 carbon

27
Q

Ethyl

A

2 carbons

28
Q

Propyl

A

3 carbons

29
Q

Butyl

A

4 carbons

30
Q

Isopropyl

A

3 carbons in a trident shape

31
Q

Polyaromatic hydrocarbons

A

Multiple aromatic rings in 1 molecule

32
Q

Alcohol

A

R-OH

33
Q

Ether

A

R’-O-R”

34
Q

Aldehyde

A

RCOH

35
Q

Ketone

A

RCOR’

36
Q

Carbonxylic Acid

A

RCOOH

37
Q

Amine

A

R-NH2

38
Q

Nitrile

A

CN

39
Q

Beer’s Law

A

Absorbance = molar absorptivity * path length * concentration

A = abc

40
Q

Qualitative analysis

A

Is it there or not?

41
Q

Quantitative analysis

A

How much is there?

42
Q

Boyle’s Law

A

P1V1 = P2V2

43
Q

Charles Law

A

V1/T1 = V2/T2

44
Q

Gay-Lussac’s Law

A

P1/T1 = P2/V2

45
Q

All the laws combined

A

V ∝ T/P

46
Q

Ideal gas law

A

PV = nRT

47
Q

Kinetic theory of gases

A
  • A gas consists of a large number of very small particles
  • Net volume of particles is negligible
  • Elastic collisions in straight lines
48
Q

Spectroscopy

A

Measures interactions of chemical w/ EMR

49
Q

Electrochemical

A

Measures interaction of chemical with electric field

50
Q

IR spectroscopy

A

Molecular vibrations and rotations from IR exposure

51
Q

Xray diffraction

A

Incident xray gives off characteristic patter

52
Q

Xray fluorescence

A

Characterstic secondary xray from incident xray

53
Q

Atomic absorption and emission spec

A

Observe emitted radiation from decay of excited compound

54
Q

Gas chromatography

A

Measures retention times of components in mobile phase in addition to quantitative analysis

55
Q

HPLC

A

similar to GC but mobile phase is liquid and is used for less volatile or more reactive chemicals

56
Q

Ion chromatography

A

Similar to HPLC but uses ion exchange resins for separation

57
Q

Ion exchange electrodes

A

Glass electrode that gives highly selective response to hydrogen ions, commonly used in pH meters

58
Q

Electron capture detectors

A

Isotope releases electrons in carrier gas towards an anode to create a current. Electron capturing analytes take an amount of those electrons, affecting the current.

59
Q

Flame ionization detector

A

Creation of organic ions by passing H2 through a flame, measuring conductivity of the flame. Used with many organic compounds.

60
Q

Photoionization detector

A

Creates ions through UV exposure, measures conductivity of gases in the light field. Used with organics, especially aromatics.

61
Q

Fick’s Law of Diffusion

A

W = D (A/L) (C1 - C0)

W = mass transfer rate
D = Diffusion coefficient
A = Frontal area of static layer
L = Length of static layer
C1 = ambient concentration
C0 = concentration at collection surface (should be 0)

CIH (11 decks)

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