Cycle 6 Chemistry

studied byStudied by 128 people
5.0(4)
Get a hint
Hint

Antoine Lavoisier

1 / 67

flashcard set

Earn XP

Description and Tags

68 Terms

1

Antoine Lavoisier

French Scientist Made a list of all 33 known elements at that time Broke into 4 categories

New cards
2

What are the 4 categories Antoine Lavoisier designated the elements to?

Gases Metals Non-Metals Earths

New cards
3

Dimitri Mendeleev

Arranged elements by increasing mass and putting elements that shared properties in columns Realized that there were undiscovered periodic elements Considered the Father of the Periodic Table

New cards
4

Henry Mosely

Arranges Elements by Atomic Number Created the Periodic Law

New cards
5

Groups

Elements in the same vertical column Otherwise known as families Numbered 1-18

New cards
6

Periods

Elements in the same horizontal row Numbered 1-7

New cards
7

Representative Elements

Elements in groups 1,2, and 13-18 (The Main Points of Reference for what we are doing)

New cards
8

Periodic Law

States that there is a periodic repetition of physical and chemical properties of the elements when arranged according to increasing atomic number

New cards
9

What are elements arranged by?

Increasing atomic number

New cards
10

Valence Electrons

Defined as electrons in the outermost orbitals of the atom

New cards
11

Metals

Shiny Solid at Room Temperature Good Conductors of heat Most elements are metals

New cards
12

Non-metals

Elements that are generally gases or brittle Poor conductors

New cards
13

Metalloids

Have physical and chemical properties of both elements 8 Metals

New cards
14

Group 1

Alkaline Metals Very Reactive

New cards
15

Group 2

Alkaline Earth Metals Very Reactive

New cards
16

Transition Metals

Similar Properties to other metals but do act a bit differently due to their partially filled subshells

New cards
17

Inner Transition Metals

The two columns at the bottom of the periodic table Lanthanides Actinides

New cards
18

Group 17

Halogens Highly reactive Very Close to becoming Noble Gases

New cards
19

Group 18

Noble Gasses Unreactive In a perfect state of balance

New cards
20

How are Groups generally identified?

By the element at the top of the group Ex. Carbon Family

New cards
21

KNOW THE DIFFERENT BLOCKS

S, D, P, F

New cards
22

Ions

Atoms of an element which gained or lost electrons

New cards
23

Anions

Atoms that gain electrons and become negatively charged. More electrons than protons Atoms get bigger as they gain more electrons

New cards
24

Cations

Atoms that lose electrons and become positively charged. Atoms get smaller as they give away their valence electron. More protons than Electrons

New cards
25

Why do Ions form?

To help increase stability of the atoms

New cards
26

Atomic Radius

The size of the atom is influenced by the number of electrons that an atom has. Atomic size is determined by how close an atom is to its neighboring atom. Definition: Half the distance between two equidistance nuclei

New cards
27

How is there an increase in atomic radius?

The atomic radius increases as you go to the left in the periodic table and down.

New cards
28

What occurs with more added Electrons?

Larger Orbital Size More Electron shielding

New cards
29

Electronegativity

Indicates the relative ability of its atoms to attract electrons in a chemical bond

New cards
30

How is there an increase in electronegativity?

As you move more to the right and up.

New cards
31

Periodic Trend

Electronegativity increases as you move to the right More protons in the nucleus to attract electrons

New cards
32

Group Trend

Electronegativity increases as you go up Strong Attraction to electrons

New cards
33

Octet Rule

Atoms tend to gain, lose, or share electrons in order to achieve stability. Aka 8 valence electrons

New cards
34

Why is the Periodic Table called the Periodic Table?

This is because the Periodic Table is periodic, meaning there is a repeating pattern with it.

New cards
35

Ionic Bonds

IONIC BONDS FORM BETWEEN METALS AND NON-METALS Ionic Bonds from when atoms become ions

New cards
36

What are Ionic Compounds Called?

Formula Units

New cards
37

Formula Units

The chemical formula of anionic compounds that lists the ions in the lowest ratio that equals a neutral electric charge.

New cards
38

DO WE USE THE WORD MOLECULE

NOOOOOOOOOOOO

New cards
39

How are ions arranged?

In a Crystal Lattice Structure

New cards
40

Crystal Lattice Structure

A repeating pattern of positive and negatively charged ions

New cards
41

Qualities of the Crystal Lattice Structure

Maximizes attraction between positive and negative ions which equal strong bonds Presence of particular metal ions lead to different colors

New cards
42

How is the STRENGTH OF IONIC BONDS MEASURED???

LATTICE ENERGY DUE TO THE CRYSTAL LATTICE STRUCTURE

New cards
43

What does Lattice energy do?

Relates the size and charge of the ions to the energy level needed to make the bond

New cards
44

Coulombs Law

Relates attraction to size and charge. Smaller atoms can be closer together and form stronger bonds. Larger atoms form smaller bonds that are weaker

New cards
45

Ionic Solids

Do not conduct electricity Charged ions can't flow and make a current

New cards
46

Ionic Solutions

When dissolved in water, they become electrolytes Conduct electricity very well Ions are separated and mixed

New cards
47

Properties of Ionic Compounds

Melting Point- Temperature that solids turn to liquids Ionic compounds have a very high melting point because of strong ionic bonds Boiling Point- Temperature at which a liquid becomes a gas. Ionic Compounds have a high boiling point

New cards
48

Ionic Compound Properties

Hard- Ionic Compounds in the solid form are hard because of strong ionic bonds that hold them together Brittle- Ionic Solids, despite being hard, are brittle of impacted with enough force.

New cards
49

What occurs everytime there is a chemical reaction?

Bonds are broken or made energy is either absorbed or released

New cards
50

Endothermic

Energy is absorbed by the chemical reaction

New cards
51

Exothermic

Energy is released by the chemical reaction THE FORMATION OF IONIC BONDS ARE ALWAYS EXOTHERMIC

New cards
52

KNOW HOW TO DO NAMING, CRISS CROSS, ETC

TRASH

New cards
53

Polyatomic Ions

Ions made with more than one atom bonded together These ions are charged molecules Act as a group

New cards
54

Metallic Bonds

Metals are not ionically bonded but share several properties with ionic compounds. Metals are arranged in crystal lattice structures in their solid states. The attraction between the positive metal cations and the negatively charged sea of electrons

New cards
55

Electronic Sea Model

The primary explanation for metallic bonding. Metals are described as having Localized metal cations (positively charged) Delocalized valence electrons (negatively charged)

New cards
56

What does the Electron Sea Model propose?

All metals contribute to their valence electrons to form a sea of electrons. The delocalized electrons are free to move around the metal cations.

New cards
57

How is the strength of a metallic bond regulated?

Related to the number of valence electrons contributed by the metal atom. The more valence electrons, the stronger the metallic bond.

New cards
58

Malleable

Metals are able to be hammered or rolled into thin sheets Ex. Aluminum foil

New cards
59

Ductile

Metals are able to be drawn into thin wires

New cards
60

Alloys

Mixtures of metals that have unique properties.

New cards
61

Substitutional Alloys

Alloys capable of taking the place of other metals because of their similar properties

New cards
62

Interstitial Alloys

Intertwined within the solids. In the smaller places electrons would reside in, but not as small as an electron.

New cards
63

How does Electron Configurations relate to the Periodic Table?

The last number in an electron configuration will match up to whatever PERIOD an element is in.

New cards
64

Atomic Size

Defined by how closely an atom lies to a neighboring atom ATOMIC SIZE AND ATOMIC RADIUS ARE DIFFERNENT

New cards
65

What happens when atoms gain electrons?

They become bigger

New cards
66

Shielding

Involving the shielding of electrons and their charge from the nucleus of an atom.

New cards
67

Nuclear Charge

Can pull electrons closer to the nucleus of an atom. The stronger it is, the more electrons can be pulled.

New cards
68

Unit Cell

The smallest arrangement of atoms in a crystal lattice structure that has the same symmetry as the whole crystal; a small representative that is part of a whole

New cards

Explore top notes

note Note
studied byStudied by 15938 people
... ago
4.9(156)
note Note
studied byStudied by 1 person
... ago
5.0(1)
note Note
studied byStudied by 53 people
... ago
5.0(1)
note Note
studied byStudied by 123 people
... ago
5.0(2)
note Note
studied byStudied by 12 people
... ago
5.0(1)
note Note
studied byStudied by 44 people
... ago
5.0(2)
note Note
studied byStudied by 90 people
... ago
5.0(2)
note Note
studied byStudied by 125845 people
... ago
4.9(606)

Explore top flashcards

flashcards Flashcard (78)
studied byStudied by 7 people
... ago
5.0(1)
flashcards Flashcard (21)
studied byStudied by 4 people
... ago
5.0(1)
flashcards Flashcard (70)
studied byStudied by 36 people
... ago
5.0(1)
flashcards Flashcard (308)
studied byStudied by 7 people
... ago
5.0(1)
flashcards Flashcard (49)
studied byStudied by 174 people
... ago
5.0(3)
flashcards Flashcard (25)
studied byStudied by 5 people
... ago
5.0(1)
flashcards Flashcard (38)
studied byStudied by 12 people
... ago
5.0(1)
flashcards Flashcard (71)
studied byStudied by 2 people
... ago
5.0(1)
robot