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Chem 101 > Part 1 Long QUIZ > Flashcards

Part 1 Long QUIZ Flashcards

1
Q

Arranged in increasing order according to atomic number

A

Periodic Table

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2
Q

Elements in same column have same number of

A

Valence electrons

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3
Q

Atomic Number = number of _______ in nucleus of an atom

A

Protons

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4
Q

Isotopes have the same number of

A

Protons

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5
Q

What elements are included in Light Elements

A

Hydrogen, Helium, Lithium, Beryllium

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6
Q

What is created from the Big Bang

A

Light Elements

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7
Q

What kind of elements after Beryllium up to iron

A

Heavy Elements

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8
Q

What are heavier elements composed of?

A

Elements that have more than the atomic number of iron

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9
Q

What charge are protons

A

Positively charged

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10
Q

What charge are neutrons

A

No charge

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11
Q

What charge are electrons

A

Negatively charged

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12
Q

Atomic Mass =

A

Protons + Neutrons

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13
Q

Neutrons =

A

Atomic Mass - Protons

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14
Q

Who used a telescope to prove nebulae were actually distant galaxies

A

Edwin Hubble (1929), Astronomer

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15
Q

Who developed the Big Bang Theory

A

Edwin Hubble

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16
Q

Who said hot, dense early universe led to the creation of light elements

A

George Gamow

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17
Q

Who proposed Big Bang Nucleusynthesis

A

George Gamow

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18
Q

Who based that there are elements and alsk expanded the idea in “αβγ paper”

A

Ralph Alpher

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19
Q

Who researched on nucleur reactions in stars thus explaining the formation of heavier elements

A

Hans Bethe

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20
Q

Not a theory, but a description of the universe

A

Big Bang

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21
Q

Big Bang is about the _________,not an explosion
Clue: Malevolent Shrine

A

Expansion of the Universe

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22
Q

Process of creating elements

A

Nucleosynthesis

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23
Q

What kind of reaction release energy

A

Exothermic Reaction

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24
Q

What kind of reaction consumes energy

A

Endothermic Reaction

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25
Reaction through light nuceli combined to form heavier nuclei
Nuclear Fusion
26
Isotope of hydrogen with one neutron
Deuteron
27
Isotope of hydrogen with two neutrons
Triton
28
Clumping of matter Formed due to high temperature Stops up to iron
Heavy Elements
29
What cycle in the life cycle of a star produces a lot of light elements From hydrogen to beryllium
Main Sequence
30
What cycle in the life cycle of a star produces light and heavy elements Hydrogen to iron
Red supergiant
31
What cycle in the life cycle of a star produces heavy and heavier elements
Supernova
32
What cycle in the life cycle of a star produces elements heavier than iron
Neutron Star
33
What elements are being produced in a black hole
NO ELEMENTS
34
Created from supernova explosions and neutron star mergers
Elements heavier than Iron
35
Key element in forming elements heavier than Iron
Neutron Capture
36
Who proposed the solid sphere model in atomic theory
John Dalton, 1803
37
All particles are made from atoms
Solid Sphere Model
38
All objects are made from atoms and they are indivisible
Solid Sphere Model
39
All atoms in the element are identical
Solid Sphere Model
40
Atoms can neither be created nor destroyed in a chemical reaction
Solid Sphere Model
41
Who proposed Plum Pudding Model
J.J. Thomson
42
Shows atoms as composed of electrons scattered throughout a spherical cloud of positive charge
Plum Pudding Model
43
Who proposed Nuclear Model
Ernest Rutherford
44
Fired positively charged alpha particles at a thin sheet of gold foil
Nuclear Model
45
Atom was mostly space, with the positive charge concentrated in the centre: nucleus
Nuclear Model
46
Electrons move around the nucelus in orbits of fixed sizes and energies
Planetary Model
47
Who proposed the planetary model
Niels Bohr
48
Electron energy in this model was quantised
Planetary Model
49
Who proposed Quantum Model
Erwin Schrödinger
50
Electrons do not move in set paths around the nucleus, but in waves
Quantum Model
51
This model proposes cloud of probability, called orbitals
Quantum Model
52
Found at the center of an atom
Nucleus
53
Where electrons orbit
Orbitals
54
Distribution of electrical charge around atoms, chemical groups, or molecule
Polarity
55
How to determine polarity
- electronegativity difference - assessing molecular shape
56
In electronegativity difference, if difference is x > 1.7, bond is
Ionic
57
In electronegativity difference, if difference is x < 0.5, bond is
Nonpolar
58
In electronegativity difference, if difference is x is greater than or equal to 0.5 but less than or equal to 1.7, bond is
Polar
59
List all molecular shapes
- linear - trigonal planar - bent or angular - tetrahedral - trigonal pyramidial - trigonal bipyramidial - octahedral
60
What molecular shape are polar and unstable
- bent or angular - trigonal pyramidial
61
Ability of an atom to attract electrons towards itself in a chemical bond
Electronegativity
62
- forces that holds the whole molecule together - found within a molecule
Intramolecular forces
63
Forces between two molecules
Intermolecular forces
64
What matter - conforms to shape of container, volume limited by surface - moderate IMF - moderate melting point and boiling point
Liquid
65
What matter - maintains own shape and volume - strong IMF - high melting point and boiling point
Solid
66
What matter - conforms to shape and volume of container - weak IMF - low melting point and boiling point
Gas
67
What do you call a positive (+) ion
Cation
68
What do you call a negative (-) ion
Anion
69
What are the four types of intermolecular forces
- Dispersion Forces (London Dispersion Forces) - Dipole-Dipole Forces - H-Bond - Ion-Dipole Forces
70
- default intermolecular force - present in nonpolar molecules & all molecules and atoms - caused by fluctuations in the electron distribution within molecules - electrons may be unevenly distributed
London Dispersion Forces
71
- attractive forces between ion and polar molecule
Ion-Dipole Forces
72
- can only exist in polar molecules - bent or angular - not dispersion due to electronegativity and shape - lone pair of a molecule is negative and is attracted to the tail of the other molecule
Dipole-Dipole Forces
73
- special type of dipole-dipole forces - must be polar and a dipole-dipole - occur when there is hydrogen being attracted to the lone pairs in another molecule - elements connected to Nitrogen, Oxygen, and Fluorine
H-bond

Chem 101 (1 decks)

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