Inorg Flashcards

Question

Ernest Rutherford 2

Answer 1

Discovered alpha beta and gamma rays in radiation

Answer 2

Developed the Schrödinger equation which describes how the quantum state of a system changes with time

Answer 3

Theorized that radioactive particles cause atoms to break down releasing radiation that take form in energy and subatomic particles

Answer 4

Discovered the radioactive elements Polonium and Radium

Answer 5

Father of Modern Chemistry

Answer 6

Named oxygen and proved that water is a compound of hydrogen and oxygen

Answer 7

Conservation of mass in a chemical reaction

Answer 8

Introduced a new system of nomenclature where each substance was given a single name which described its composition

Answer 9

Formulated the Avogadro's law and Avogadro's number 6.022x10^23

Answer 10

Isolated new elements and developed a chemical notation system using letters and numbers

Answer 11

Created 36 chemical symbols

Answer 12

First to describe atoms in a modern scientific sense

Answer 13

Showed the existence of protons and electrons

Answer 14

Showed the nucleus

Answer 15

Showed energy levels

Answer 16

Showed subshells and shells are actually orbitals

Answer 17

Existence of neutrons

Answer 18

Number of protons and neutrons in an atom

Answer 19

Number of protons in an atom

Answer 20

Abbreviation used to represent atom in chemical formulas

Answer 21

Discovered isotopes

Answer 22

Proposed the law of Triads where the middle element in certain triads had an atomic weight that was average of the other two members

Answer 23

Law of Octaves where every eighth element shared similar properties

Answer 24

Studied the relationship of the atomic volume and relative atomic mass of 28 elements

Answer 25

Formulated Periodic Law and made a periodic table of 63 known elements where their properties are periodic functions of their atomic masses

Answer 26

First suggested that the number of charges in an element's atomic nucleus is exactly equal to the element's place on Mendeleev's table

Answer 27

Discovered atomic number and its relationship between atomic mass

Answer 28

Discovery of 10 transuranium elements

Answer 29

Had an element named after him while he was still alive

Answer 30

Gold/light yellow

Answer 31

Silver and white

Answer 32

Blue violet

Answer 33

Red to violet

Answer 34

Had an element named after him while he was still alive ## Footnote Example: Seaborgium (Sg)

Answer 35

International Union of Pure and Applied Chemistry

Answer 36

Lustrous soft and highly reactive metals ready to form +1 cations and found naturally only in salts

Answer 37

React with water to form alkaline hydroxides readily lose valence to form +2 cations

Answer 38

Less reactive than group 1 and 2 metals have higher melting points and densities

Answer 39

Have low melting points and poor hardness and react with oxygen to form oxides

Answer 40

Has four valence electrons form hydrides with hydrogen tetrahalides with halogens and variety of oxides with oxygen

Answer 41

Have five valence electrons all are solid except the first element

Answer 42

Have six valence electrons and electronegative nonmetals react with metals to form -2 ions

Answer 43

All are reactive nonmetals have seven electrons and only group that contains solid liquid and gas (I and As are solids Br is liquid and F and Cl are gases)

Answer 44

Very low chemical reactivity and colorless gases but exhibit colors when ionized

Answer 45

B, Si, Ge, As, Sb, Te

Answer 46

One of two or more distinct forms of an element

Answer 47

Stock nomenclature where oxidation states are indicated in parentheses by Roman numerals

Answer 48

Compounds that have specific number of water molecules attached to them

Answer 49

Contains a hydrogen and an anion

Answer 50

Contains a hydrogen and an oxyanion

Answer 51

Na2CO3 • 10H2O

Answer 52

CaMg(CO3)2

Answer 53

Na2SO4 • 10H2O

Answer 54

MgSO4 • 7H2O

Answer 55

CaSO4 • 1/2 H2O

Answer 56

CaSO4 • 2H2O

Answer 57

CuSO4 • 5H2O

Answer 58

FeSO4 • 7H2O

Answer 59

ZnSO4 •7H2O

Answer 60

Identified the first

Answer 61

H2SO4 ## Footnote Sulfuric acid

Answer 62

CuSO4 • 5H2O ## Footnote Copper(II) sulfate pentahydrate

Answer 63

FeSO4 • 7H2O ## Footnote Iron(II) sulfate heptahydrate

Answer 64

ZnSO4 • 7H2O ## Footnote Zinc sulfate heptahydrate

Answer 65

B2H6 ## Footnote Diborane is a colorless, highly reactive gas

Answer 66

SiH4 ## Footnote Silicon tetrahydride

Answer 67

PH3 ## Footnote Phosphine is a colorless, flammable gas

Answer 68

H2S ## Footnote Hydrogen sulfide is a colorless gas with a characteristic odor of rotten eggs

Answer 69

Identified the first example of isomerism and that nitrogen is an essential plant nutrient ## Footnote Chemist and principal founder of organic chemistry

Answer 70

Accidentally synthesized urea and co-discoverer of Be and Si ## Footnote German chemist known for his discovery of the synthesis of urea

Answer 71

Structure of benzene's ring shaped structure ## Footnote German chemist who proposed the structure of benzene

Answer 72

Used X-ray crystallography to prove the benzene ring's structure ## Footnote Irish crystallographer and first woman tenured professor at University College London

Answer 73

Known for his work on chemical bonding and proposed the Pauling electronegativity scale ## Footnote American chemist and two-time Nobel Prize winner

Answer 74

Faraday's constant 96485 C/mol ## Footnote English scientist who contributed to the fields of electromagnetism and electrochemistry

Answer 75

Pioneers of organometallic chemistry and pioneered the concept of combining power or valence ## Footnote English chemist known for his work on valence theory

Answer 76

First winner of the Nobel prize in Chemistry and one of the founders of physical chemistry laid foundation for stereochemistry ## Footnote Dutch physical chemist and first winner of the Nobel Prize in Chemistry

Answer 77

Lewis structure ## Footnote American physical chemist known for his concept of electron pairs

Answer 78

Developed the Hückel method of approximate molecular orbital calculations on π electron systems ## Footnote German physical chemist and physicist

Answer 79

Discovered Grignard reagent and reaction ## Footnote French chemist and Nobel Prize winner

Answer 80

Discovered Fischer esterification developed Fischer projection and hypothesized lock and key mechanism of enzyme action ## Footnote German chemist and Nobel Prize winner

Answer 81

Combination of two or more atomic orbitals to form the same number of hybrid orbitals each having the same shape and energy ## Footnote Concept in chemistry to explain the geometry of molecules

Answer 82

Bond strength decreases ## Footnote Inverse relationship in chemical bonds

Answer 83

Electronegative difference is less than 0.4 ## Footnote Type of covalent bond with equal sharing of electrons

Answer 84

Electronegative difference is 2.0 or more ## Footnote Type of bond formed between a metal and a non-metal

Answer 85

Electronegative difference between 0.4-1.7 ## Footnote Type of covalent bond with unequal sharing of electrons

Answer 86

The pull of electron density through sigma bonds caused by electronegativity difference of atoms ## Footnote Effect in organic chemistry that influences the distribution of electrons

Answer 87

Two rings share one atom, has the prefix spiro[x.y] where x is smaller ## Footnote Type of bicyclic compound

Answer 88

Two rings share two atoms in one bond, bicyclo[x.y.0] where x is bigger ## Footnote Type of bicyclic compound with shared atoms

Answer 89

Two rings share three or more atoms, separating the two bridgehead atoms by a bridge containing at least one atom, bicyclo[x.y.z] where x is bigger and z is number of bridgehead atoms ## Footnote Type of bicyclic compound with a bridge

Answer 90

Alkyl halide < ether < alkane < alkyne < alkene < amine < alcohol < ketone < aldehyde < nitrile < amide < ester < carboxylic acid ## Footnote Order of priority for functional groups in organic chemistry

Answer 91

Distance between identical points on consecutive waves ## Footnote Physical property of a wave

Answer 92

Distance between origin and crest or trough ## Footnote Measure of the height of a wave

Answer 93

Number of waves that pass per unit time ## Footnote Measure of the rate of wave oscillation

Answer 94

Wavelength times frequency ## Footnote Relationship between wavelength and frequency in waves

Answer 95

3x10^8 m/s ## Footnote Constant speed of light in a vacuum

Answer 96

Relationship between an object's temperature and the wavelength of electromagnetic radiation it emits ## Footnote Thermal radiation from a perfect absorber and emitter of electromagnetic radiation

Answer 97

E = hv = (hc)/lambda ## Footnote Equation describing the energy of a photon

Answer 98

h= 6.626x10^-34 J•s/particle ## Footnote Physical constant used in quantum mechanics

Answer 99

Blue ## Footnote Color of flame produced by burning indium

Answer 100

Light blue ## Footnote Color of flame produced by burning lead

Answer 101

Blue ## Footnote Color of flame produced by burning arsenic

Answer 102

Blue ## Footnote Color of flame produced by burning sulfur

Answer 103

Crimson red ## Footnote Color of flame produced by burning radium

Answer 104

Pale green ## Footnote Color of flame produced by burning antimony

Answer 105

Azure blue ## Footnote Color of flame produced by burning selenium

Answer 106

Blue-white ## Footnote Color of flame produced by burning tin

Answer 107

Blue ## Footnote Color of flame produced by burning tantalum

Answer 108

Blue-green ## Footnote Color of flame produced by burning zinc

Answer 109

Green ## Footnote Color of flame produced by burning tungsten

Answer 110

Carmine crimson or scarlet red ## Footnote Color of flame produced by burning yttrium

Answer 111

Mid/dull red ## Footnote Color of flame produced by burning zirconium

Answer 112

Irradiating a metal surface causes ejection of electron ## Footnote Phenomenon where light causes emission of electrons from a material

Answer 113

Minimum energy required to remove electrons from the metal surface ## Footnote Energy required to remove an electron from a material

Answer 114

Minimum frequency multiplied by Planck's constant to obtain work function ## Footnote Frequency of light required to overcome the work function of a material

Answer 115

n main energy level and distance if electrons from nucleus ## Footnote Quantum number in atomic theory indicating main energy levels

Answer 116

l energy subshells and shape of orbitals ## Footnote Quantum number indicating energy subshells in an atom

Answer 117

Number of orbitals in subshells and possible orientation of orbitals in space ## Footnote Quantum number indicating orbital orientations

Answer 118

Movement of electron around its own axis clockwise and counterclockwise ## Footnote Quantum number indicating electron spin

Answer 119

Building up principle orbital with lower energy is filled up first ## Footnote Principle in chemistry for filling electron orbitals

Answer 120

Energy increases with increasing n + 1 ## Footnote Rule for determining electron configurations

Answer 121

For degenerate orbitals electrons must first occupy them singly with parallel spin before filling with pairs ## Footnote Rule for filling electron orbitals

Answer 122

No two electrons can have the same set of quantum numbers ## Footnote Principle in quantum mechanics

Answer 123

[Ar] 4s1 3d5 ## Footnote Electron configuration of Chromium

Answer 124

[Kr] 5s1 4d5 ## Footnote Electron configuration of Molybdenum

Answer 125

[Ar] 4s1 3d10 ## Footnote Electron configuration of Copper

Answer 126

[Kr] ## Footnote Electron configuration of Silver

Answer 127

For degenerate orbitals electrons must first occupy them singly with parallel spin before filling with pairs ## Footnote Example: In the 2p subshell, each electron will first occupy a separate orbital before pairing up

Answer 128

No two electrons can have the same set of quantum numbers

Answer 129

[Ar] 4s1 3d5

Answer 130

[Kr] 5s1 4d5

Answer 131

[Ar] 4s1 3d10

Answer 132

[Kr] 5s1 4d10

Answer 133

Used to calculate the shielding constant

Answer 134

Additional electrons do not add to the atomic size in the 5th and 6th period

Answer 135

Energy required to remove an electron from a gaseous atom in its ground state

Answer 136

Energy change associated with the addition of an electron to a gaseous atom in its ground state

Answer 137

Ability to be distorted by an electric field

Answer 138

Larger species = greater polarizability

Answer 139

Square pyramidal

Answer 140

Square Planar

Answer 141

Quantitative measure of bond polarity

Answer 142

μ= Q x r where Q is charge r is distance and μ is expressed in (D) Debye units

Answer 143

Weak forces of attraction as a result of nonsymmetrical electron distribution that created a temporary dipole moment

Answer 144

Occurs between compounds with permanent dipole moment

Answer 145

Only occurs when H is bonded to N O or F

Answer 146

Between compounds with positive and negative charges

Answer 147

Small highly charged cations have polarizing ability Large highly charged anions are easily polarized Cations that do not have a noble-gas electron configuration are easily polarized

Answer 148

Attraction between electropositive atoms and delocalized electrons within a metal lattice

Answer 149

Attraction resulting from the sharing of electrons of atoms

Answer 150

Produces H+ in aqueous solution

Answer 151

Produces OH- in aqueous solution

Answer 152

Proton donor

Answer 153

Proton acceptor

Answer 154

Electron pair acceptor

Answer 155

Electron pair donor

Answer 156

Acidic proton is on a water molecule coordinated to a central metal ion

Answer 157

Acidic proton is on a hydroxyl group without a neighboring oxo group

Answer 158

Acidic proton is on a hydroxyl group with an oxo group attached to the same atom

Answer 159

Hard acid bind to hard base and soft acid bind to soft base

Answer 160

Smaller, high charge and highly polarizing

Answer 161

Bigger, low charge, and low polarizing

Answer 162

Smaller high charge least polarizable

Answer 163

Big low charge highly polarizable

Answer 164

Molecules with at least one unpaired electron

Answer 165

Molecules with fully paired electrons

Answer 166

Permanent magnet

Answer 167

The highest symmetry axis in a molecule

Answer 168

Solids with highly regular arrangements of their components

Answer 169

Solids with considerable disorder in their structures

Answer 170

Number of nearest nearby atoms in a lattice

Answer 171

When valence band and conduction band overlap

Answer 172

A large band gap between the valence and conduction band which prevents the motion of electrons

Answer 173

The band gap is small enough that energy may be inputted to excite valence band electrons to the conduction band

Answer 174

Elements that exhibit semi-conductive behavior at their pure state

Answer 175

Group 15 elements are capable of adding an electron relative to the host semiconductor

Answer 176

Group 13 elements provide a positive hole for increasing conductance

Answer 177

A mixture of metals or a mixture of a metal and another elements

Answer 178

Some of the host metal atoms are replaced by other metal atoms of similar size

Answer 179

Formed when some of the interstices or holes in the closest packed metal structure are occupied by small atoms

Answer 180

Has discrete molecular units at each lattice position

Answer 181

Have atoms occupying the lattice points

Answer 182

Stable high-melting substance held together by strong electrostatic forces that exist between oppositely charged ions

Answer 183

The change in energy that takes place when separated gaseous ions are packed together to form an ionic solid

Answer 184

Transition metals (Lewis acid) accept electrons from ligands (Lewis base)

Answer 185

Oxidation state of metal

Answer 186

Coordination number

Answer 187

Number of times a ligands binds to a metal through donor atoms

Answer 188

Only occurs with ambidentate ligands where the same ligand may link through different atoms

Answer 189

the change in energy that takes place when separated gaseous ions are packed together to form an ionic solid

Answer 190

coordination number

Answer 191

number of times a ligands binds to a metal through donor atoms

Answer 192

only occurs with ambidentate ligands where the same ligand may link through different atoms

Answer 193

occurs when a ligand and a counterion in one compound exchange places

Answer 194

Ionization isomer but is specific for water

Answer 195

arises when there are different complex ions that can form the same molecular formula, or simply two metals exchanging ligands

Answer 196

denote complexes which have the same empirical formula but different molar masses

Answer 197

isomers differing only in their three-dimensional arrangement

Answer 198

non-superimposable mirror images of each other and can rotate plane-polarized light

Answer 199

electrostatic model that involves interactions between the electrons from the ligands and the electrons in the metal d-orbitals

Answer 200

The separation of the two sets of orbitals ## Footnote The magnitude of the ligand field splitting parameter depends on the charge on the metal ion principal quantum number and the nature of the ligand

Answer 201

shorter metal-ligand distance, stronger orbital-ligand interaction, ∆0 increases

Answer 202

I- < Br- < SCN- < Cl- < NO3- < F- < OH- < H2O < NCS- < NH3 < en < phen < NO2- < PPh3 < CN- < CO

Answer 203

if color absorbed is red, color seen is green

Answer 204

if color absorbed is yellow, color seen is violet

Answer 205

acids that yield more than one H3O+ ion

Answer 206

combination of a weak acid/base and its conjugate acid/base in equal concentrations

Answer 207

Gain electrons reduction oxidizing agent

Answer 208

lose electrons oxidation reducing agent

Answer 209

total number of electrons removed/added to an element

Answer 210

All matter is made up of indestructive units called atoms ## Footnote Example sentence: Democritus was an ancient Greek philosopher who proposed the concept of atoms.

Answer 211

Proposed the idea of quantization

Answer 212

Chemical reactions involve reorganization of the atoms

Answer 213

Each element is made up of atom

Answer 214

Atoms of a given compound are identical

Answer 215

Compounds are formed when atoms combine with each other

Answer 216

Discovered that there appeared to be more than one element at each position on the periodic table

Answer 217

Coined the term isotope

Answer 218

Created the periodic table based on the periodic functions of their atomic weight

Answer 219

Found that noble gases have stable electron configurations

Answer 220

Proposed the theory of electromagnetism and made connection between light and electromagnetic waves

Answer 221

Created the theories of relativity and hypothesized about the particle nature of light

Answer 222

Proposed that electricity was made up of discrete negative particles called electrons

Answer 223

Invented a device that could detect alpha particles

Answer 224

Demonstrated in his experiments that cathode rays have a negative charge

Answer 225

Determined the charge of an electron through his oil drop experiment

Answer 226

Used cathode ray tube to study canal rays which had electrical and magnetic properties opposite of an electron

Answer 227

Performed alpha particle experiment and established that the nucleus was very dense very small and positively charged

Answer 228

Discovered that certain chemicals glowed when exposed to cathode rays called X-rays

Answer 229

Discovered that the number of protons in an element determines its atomic number

Answer 230

Discovered radiation by studying the effects of X-rays on photographic film

Answer 231

Developed Bohr atomic model with electrons travelling in orbits around the nucleus

Answer 232

Used cathode ray tubes to determine the charge to mass ratio of an electron

Answer 233

Proposed that electrons have a wave-particle duality

Answer 234