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General Chemistry Stuff Flashcards

(86 cards)

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1
Q

Definition of Chemistry

A

the study of matter and the changes it undergoes

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2
Q

Definition of matter

A

anything that has mass and takes up space

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3
Q

Definition of atoms

A

submicroscopic particles that are the fundamental “building blocks” of all matter

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4
Q

Physical characteristics of solid

A
  • definite shape
  • not easily compressible
  • molecules are densely packed
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5
Q

Physical characteristics of liquid

A
  • no definite shape
  • not easily compressible
  • molecules are loosely packed
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6
Q

Physical characteristics of gas

A
  • no definite shape
  • easily compressible
  • molecules not packed
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7
Q

An tank of gas becomes “empty” when -

A

the pressure inside the tank equalizes with the pressure of the atmosphere (even if there is still gas in the tank)

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8
Q

Atomic mass

A

Made up of the protons and neutrons

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9
Q

The number of protons gives us it’s___ and identifies which ___ it is

A

atomic number; element

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10
Q

What does changing the number of neutrons of an element do?

A

change the mass and creates isotopes

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11
Q

What determines the charge of the element?

A

The electrons

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12
Q

Definition of a molecule

A

two or more atoms joined together

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13
Q

Definition of a compound

A

a molecule that contains at least two different elements

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14
Q

What is matter called that consists of two or more pure substances that retain their individual identities?

A

a mixture

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15
Q

What is a pure substance that can be broken into separate parts called?

A

a compound

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16
Q

What are chemical properties of matter?

A

property displayed by a substance caused by a change in it’s composition (flammability, acidity, toxicity)

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17
Q

Where are alkali metals found?

A

Group 1

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18
Q

Where are alkaline earth metals found?

A

Group 2

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19
Q

Where are halogens found?

A

Group 17

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20
Q

Where are noble gasses found?

A

Group 18

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21
Q

Where are transition metals found?

A

Group 3-12

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22
Q

What are core electrons?

A

innermost electrons that occupy the lowest energy levels and are not involved in chemical bonding

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23
Q

What are valence electrons?

A

outermost electrons that occupy the highest energy level and are involved in chemical bonding

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24
Q

Aufbau principle

A

an electron occupies the lowest-energy orbital that can receive it

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25
Trends of atomic size on periodic table
increases going down and to the left
26
Trends of electronegativity on periodic table
decreases going down and to the left
27
Empirical formula
the simplest whole number ratio of the elements in a compound
28
Structural formula
the exact number of each type of element and exact manner in which these atoms are bound together (Lewis structure)
29
Molecular formula
the exact numbers of each type of element found in a compound
30
Define atomic elements
elements that exist in nature with single atoms as their basic unit (Na, Mg, Ag, Au)
31
Define molecular elements
elements that exist in nature as molecules (H2, N2, O2, Cl2, Br2, P4)
32
What is a molecular compound?
composed of two or more non-metals
33
Melting
Solid--> liquid
34
Freezing
Liquid--> solid
35
Vaporization
Liquid --> gas
36
condensation
gas--> liquid
37
deposition
gas--> solid
38
sublimination
solid--> gas
39
Atoms
Submicroscopic particles that are the fundamental building blocks of all matter
40
What makes up the bulk of an atoms mass?
Protons and neutrons
41
Where are protons, neutrons and electrons located?
Protons and neutrons are in the nucleus. Electrons reside in the space around atoms (electron cloud)
42
What is an element?
Cannot be separated into simpler substance
43
What is a compound?
Substance composed of two or more elements. Can be separated into simpler substances/elements only by chemical methods
44
What is a homogeneous mixture?
A mixture with uniform composition (solution)
45
What is a heterogeneous mixture?
Mixture not uniform and composition and properties
46
What is a pure substance?
Cannot be broken down further
47
What is the chemical change?
A change that alters composition Creating different substances
48
Who developed the atomic theory?
John Dalton in 1808
49
Atomic theory
Each element is composed of atoms All atoms of an element have same mass and other properties that distinguish them from other atoms Atoms combine in simple whole number ratios to form compounds Atoms of one element cannot change into atoms of another element
50
Pauli exclusion principle
No 2 electrons can be the same and must be paired opposite (spin paired)
51
S-orbital
Holds 2 electrons
52
P-orbital
3 orbitals Holds 6 electrons
53
D orbitals
5 orbitals Holds 10 electrons
54
F- orbitals
7 orbitals holds 14 electrons
55
Why do atoms gain/lose electrons?
To give electron configuration similar to noble gas (more stable)
56
Cations
Lose electrons Cations are smaller than corresponding atoms
57
Anions
Gain electrons Anions are bigger than corresponding atoms
58
Non- metals
Do not conduct electricity Ex: most gases
59
Metals
Malleable/ductile Conduct electricity Usually solid (except Hg)
60
Metalloids
Properties of both metals and nonmetals
61
Neutrons
Isotope- number of protons
62
Law of conservation of mass
Lavoisier—matter is neither created nor destroyed matter is converted into other forms not destroyed
63
Law of definite proportions
All samples of a given compound have the same proportions of their constituent elements Ex: water (however it got there all water is 2H+ and 1O
64
Toxicity
An example of chemical property
65
Law of multiple proportions
When two elements form two different compounds with similar bonding Masses of element b that combine with the same amount of element A can be expressed as a ratio of small whole number
66
Example of chemical change
Iron rusting—iron rebinding to O2 changes chemical properties
67
Diatomic elements
“Have No Fear Of Ice Cold Beer” H2 N2 F2 O2 I2 Cl2 Br2
68
Ionic compound
Metal (cation) and nonmetal (anion)
69
Molecular compounds
2 or more nonmetals
70
What is Zn ion
Zn2+
71
What is Ag ion
Always Ag+
72
What is the only poly atomic cation?
Ammonium NH4+
73
How to determine ionic charge of transition metal?
Cation charge= -(anion subscript)(anion charge)/ (cation subscript)
74
Binary acids
HCl: hydrochloric acid HBr: hydrobromic acid HI: hydroiodic acid HF: hydrofluoric acid
75
Oxoacids
Come from polyatomic ions -ate goes to -ic -ite goes to -ous
76
Reducing chemical formulas
CAN reduce ionic compounds CANNOT reduce molecular compounds—would change compound
77
Why do atoms form bonds?
To lower potential energy(more stable)—high energy things are unstable Bonds allow unpaired electrons to become paired
78
Polar covalent bond
Electrons not shared equally Electron density more towards most electronegative atom
79
Nonpolar covalent bonds
Electrons are shared equally between atoms Usually when electronegativity is low Ex: C bonds, 2 of some element bonded together
80
Exceptions to octet
H: 2 electrons B: 6 electrons Al: 6 electrons
81
Expanded octets
Period 3 or higher Due to D orbitals
82
Lone pairs
Lone pairs have greater density than peripheral atoms—repel each other
83
If octahedral has lone pair which axis is it drawn on
Lone pairs fill axial axis
84
If trigonal bipyramidal have a lone pair where does it go first?
Equatorial axis fill with lone pairs
85
Binary ionic
Cation and anion are both one element ex: NaCl
86
Electronegativity
Property for bonding and reactivity

Chemistry (18 decks)

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