IB Enviro Systems- everything to memorize

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Nitrite

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so far only structure 1- the first 44 slides of 2.2

108 Terms

1

Nitrite

NO2-

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2

Nitrate

NO3-

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3

Hydroxide

OH-

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4

Hydrocarbonate

HCO3-

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5

Carbonate

CO32-

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6

Sulfite

SO32-

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7

Sulfate

SO42-

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8

Phosphite

PO33-

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9

Phosphate

PO43-

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10

Ammonium

NH4+

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11

180

  • 2 electron domains

  • linear electron domain geometry

  • 2 bonding electron domains

  • 0 pairs of non-bonding electrons

  • linear molecular geometry

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12

120

  • 3 electron domains

  • planar triangular electron domain geometry

  • 3 bonding electron domains

  • 0 pairs of non-bonding electrons

  • planar triangular molecular geometry

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13

117

  • 3 electron domains

  • planar triangular electron domain geometry

  • 2 bonding electron domains

  • 1 pair of non-bonding electrons

  • V-shaped molecular geometry

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14

109.5

  • 4 electron domains

  • tetrahedral electron domain geometry

  • 4 bonding electron domains

  • 0 pairs of non-bonding electrons

  • tetrahedral molecular geometry

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15

107

  • 4 electron domains

  • tetrahedral electron domain geometry

  • 3 bonding electron domains

  • 1 pair of non-bonding electrons

  • pyramidal molecular geometry

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16

105

  • 4 electron domains

  • tetrahedral electron domain geometry

  • 2 bonding electron domains

  • 2 pairs of non-bonding electrons

  • V-shaped molecular geometry

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17

Atom

smallest particle representing an element

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18

Element

made of one type of atom

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19

molecule

bonded nonmetals (monoatomic, diatomic or polyatomic)

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20

compound

bonded atoms that are different

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21

What Are the Diatomics

  • Iodine

  • Hydrogen

  • Nitrogen

  • Bromine

  • Oxygen

  • Chlorine

  • Flourine

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22

Water Formula

H2O

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23

Carbon Dioxide

CO2

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24

Methane

CH4

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25

Sulfuric Acid

H2SO4

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26

Calcium Carbonate

CaCO3

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27

Sodium Chloride

NaCl

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28

Hydrochloric Acid

HCl

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29

Ammonia

NH3

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30

Substances

  • uniform chemical composition

  • made of one atom or one type of compound

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31

Mixtures

  • non-unform chemical composition

  • made up of more than one substance mixed together.

  • either homogenous or heterogenous

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32

Mass number

# of protons + # of neutrons

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33

RAM equation

RAM= [(mass no. x percent abundance) + (mass no. x percent abundance)…]/100

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34

Percent abundance formula

(Mass of Isotope/average atomic mass) x 100%

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35

Heisenberg’s Uncertainty Principle

we cannot know where an electron is at any given moment in time, we only know the probable location.

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36

Wave-particle duality

electrons behave as both particles and waves (which are continuous in motion)

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37

The electromagnetic spectrum (from left to right)

Radio waves{ Micro-waves{ Infrared radiation{ Visible light{ UV{ X-rays{ Gamma-rays

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38

Wavelength

the distance between the crests or the distance between troughs

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39

Frequency

the number of wave cycles to pass during a given unit of time

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40

Amplitude

the waves height from 0 to the crest

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41

Crest

top of the wave

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Trough

bottom of the wave

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43

High frequency relates to:

short wavelength and high energy

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44

low frequency relates to:

long wavelength, low energy

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45

Color spectrum from left to right

ROYGBV (red orange yellow green blue violet)

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46

All waves travel at what speed

the speed of light ( equation c=frequency x wavelength)

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47

Energy level characteristics

  • not equidistant, they’re closer the further away from the nucleus

  • Visible light n=2

  • infrared n= 3

  • UV n=1

    • they increase in energy the farther away from the nucleus they are

      • electrons are excited and rise in energy levels then go back to their ground state

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48

Groups

columns and says the number of valence electrons in the atoms of group

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49

Periods

Rows and it’s the numbers of energy levels electrons occupy at ground state for the atoms of that element

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50

Ion

an atom that has a positive or negative charge and they form when they lose or gain electrons

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51

Cations

Lose electrons and is an ion with a positive charge

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52

Anions

Gains electrons and is an ion with a negative charge

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53

When an electron is in an orbital of higher energy…

it is most likely far from the nucleus

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54

Atomic orbitals charecteristics:

  • 3 dimensional areas where there is a high probability that the electron will be located

  • S orbitals are spherical

  • P orbitals are dumbbell-shaped

  • there are 3 orbitals located on an x, y, and z axis

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55

Aufbau Principle

lowest energy orbitals are filled first

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56

Pauli exclusion principle

up to 2 electrons can occupy an orbital but they must have an opposite spin to reduce repulsion (up arrow is clockwise, down arrow is counter clockwise)

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57

Hund’s rule

electrons are placed in orbitals of a sublevel one electron at a time

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58

electron configuration of ions

  • cations: determined by subtracting electrons that the ion loses out of the outermost occupied orbitals of its neutral configuration

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59

scientific notation

the coefficient must be greater than or equal to 1 and less than 10 and must contain all the significant digits in the number, the exponent expresses places the number is moved (negative is left and positive is right)

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60

What is avogadros number

6.02214076 × 10²3

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61

conversion between moles and rep. particles

1 mole= Avg. constant rep. particles

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62

mol of gas at stp conversion

1 mol of any gas= 22.7 dm³

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63

Temperature conversions

Kelvin from Celcius = 0C+ 273.15K

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64

what is standard pressure and standard temperature (STP)

  • standard temperature 273 K or 0 C

    • Standard pressure 100 kPa

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65

What is the limiting reactant (LR)

the reactant in the reaction that will run out

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66

what is the excess reactant

the reactant in excess (you will not run out of it)

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67

Mole ratio

a conversion factor derived from the coefficients of a balanced chemical equation that helps you convert from one reactant or product in the balanced equation to another

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68

Titration equations

  • C1V1/N1 = C2V2/N2

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69

Gas law/ ideal gases equation

PV= nRT

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70

Analyze the units of PV=nRT

P= in Pa NOT kPa

V= must be in m³

n= moles

R- constant, 8.31

T= must be in K (C + 273.15)

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71

ionic compounds

are made up of cations and anions and are a FOA between cations and anions

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72

Metallic substances

made up of metals only. Are the FOA between metal cations and delocalized valence electrons

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73

Covalent substances

made up of non-metals only. Are the FOA between nuclei and shared electrons

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74

Redox reactions

a chemical reaction in which changes in the oxidation states of a species occur throughout the reaction

oxidation= increase of oxidation state

reduction= decrease of oxidation state

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75

Oxidation state

value we assign to an atom in a compound to measure the electron control, density or possession that the atom has relative to when it is alone as a pure element

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76

Atoms in the free (uncombined) element have an oxidation state of:

zero

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77

In simple ions, the oxidation state is the:

same as the charge on the ion ex.. Mg2+, oxidation state is +2

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78

The oxidation states of all the atoms in a neutral compound must:

add up to zero

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79

The oxidation states of all the atoms in a polyatomic ion must:

add up to the charge of the ion

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80

The usual oxidation state for an element is:

the same as the charge on its most common ion ex. group 1 elements have oxidation state +1 (H is usually +1)

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81

Most main group non-metals and transition metals have oxidation states that:

vary in different compounds depending on the conditions and other elements present

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82

Oxidation state rules of O

it’s -2 except in peroxides where it is -1 and OF2 where it is +2

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83

Oxidation state rules of H

it’s +1 except metal hydrides where is it -1

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84

Oxidation state rules of Cl

it’s -1 except when it’s combined with O or F

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85

Ionic compounds have what structure:

lattice structure

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86

Describe the ionic lattice structure

  • 3-d

  • crystalline

  • FOA of ionic compounds cause them to surround themselves with ions of the opposite charge

  • ionic bonds are non-directional

  • Layout of lattice depends of size of the ions but always is based on a repeating unit

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87

Ionic bond physical properties

  • high melting points and boiling points

  • low volatility

    • both because of the strength of the bonds

  • solids at room temperature

  • generally soluble in polar solvents but not in nonpolar solvents

  • don’t conduct when in solid state

  • usually brittle

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88

solubility

the ease with a solid (the solute) dissolves in a liquid (the solvent) to form a solution

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89

Lattice enthalpy is:

the change in enthalpy (the total energy in a substance) and it tells us how strong the ionic bonds are in a lattice, to break or weaken the FOA is considered an endothermic process

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90

high lattice enthalpy takes a ____ amount of energy to weaken/break the FOA between the ions

large

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91

low lattice enthalpy takes a ____ amount of energy to weaken/break the FOA between the ions

small

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92

Factors that affect lattice anthalpy:

  • ionic radius (greater radius, lower enthalpy)

  • ionic charge (grater charge, greater enthalpy)

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93

Atomic radius

it’s the half distance between the nuclei of 2 bonded identical atoms (ex. H2)

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94

Effective nuclear charge

the net positive charge from the nucleus that an electron can “feel” attraction from. Increases across a period and decreases down a group

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95

electron shielding

core electrons shield the valence from the full attractive forces of the protons in the nucleus. Stays the same across a period and increases down a group

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96

electron repulsion

electrons repel each other because of their same charge, this causes the electron cloud to expand

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97

Ionic radius trands:

increases across a period, increases down a group

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98

First ionization energy

the amount of energy required to remove the first valence electron from one gaseous atom, depends on how strong the FOA is between the nucleus and the valence electrons of an atom

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99

electronegativity 1.8 categories

ionic compounds >1.8 electronegative difference

covalent compounds <1.8 electronegative difference

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100

In covalent bonds, the shared electrons sit..

between the nuclei of the nonmetal atoms

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