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Chemistry ICA > Periodic Table Trends and Compounds Study Guide Unit 2 > Flashcards

Periodic Table Trends and Compounds Study Guide Unit 2 Flashcards

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1
Q

Alkali Metals

A

Group 1A (Li, Na, K, Rb, Cs, Fr) except hydrogen

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2
Q

Alkaline Earth Metals

A

Group 2A (Be, Mg, Ca, Sr, Ba, Ra)

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3
Q

Halogen

A

Group 7A highly Reactive

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4
Q

Noble Gases

A

Group 8A Highly Unreactive Group

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5
Q

Transition Metals

A

Group B (in the middle)

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6
Q

Inner Transition Metals

A

Group B

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7
Q

ionization energy

A

The energy required to make an ion by removing an electron

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8
Q

Cation

A

Atom or group of atoms that has a positive charge

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9
Q

Anion

A

Atom or group of atoms that has a negative charge

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10
Q

Electronegativity

A

The tendency of atoms of the element to attract electrons

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11
Q

Molecule

A

Combination of a nonmetal and nonmetal NEED PREFIX

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12
Q

Formula Unit

A

Combination of a metal and nonmetal NO PREFIX

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13
Q

Ionic Compound

A

A force that holds oppositely charged particles together

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14
Q

Covalent Bond

A

The bond formed when two nonmetal atoms share electrons

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15
Q

Polyatomic Ion

A

Group of Atoms that have a positive and negative charge

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16
Q

octet rule

A

Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas usually eight valence electrons

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17
Q

Atomic size TRENDS

A
  1. Periodic Trend from LEFT to RIGHT down electrons are the same distance but are closer to the nuclei
  2. Group Trend going Down because outer electrons are in further energy levels
  3. The radius is C=0.77 A
18
Q

Ionic Size TRENDS

A
  1. Decreases in size from left to right for both cations and anions (periodic)
  2. Group trend-increases in size going down
19
Q

When do cations form

A

when an atom loses electrons

20
Q

When do anions form

A

when an atom gains electrons

21
Q

Factors of Ionizing Energy

A
  1. number of electrons (further the valence electrons are easier to pull off the electron)
  2. Shielding Effect (inner electrons decrease the effective nuclear charge)
  3. Size of the Nucleus ( the bigger the stronger the pull)
22
Q

Ionizing Energy TRENDS

A
  1. Periodic- increases from left to right, electrons are the same distance but are pulled tighter by bigger nuclei
  2. Group- decreases from top to bottom because electrons are farther away and are shield by inner electrons
23
Q

Electronegativity Trends

A
  1. Periodic- increases from right to left

2. Group- decreases going down

24
Q

Where are Alkali Metals and What are they

A

ALL the way on the Left (Li, Na, K, Rb, Cs, Fr) DO NOT INCLUDE Hydrogen

25
Q

Where are Alkaline Earth Metals and What are they

A

The column next to the Alkali Metals ( Be, Mg, Ca, Sr, Ba, Ra)

26
Q

Where are Halogens and What are they

A

5th row in the known metals (F, Cl, Br, I, At)

27
Q

Where are Noble gases and What are they

A

The last row in the periodic table (He, Ne, Ar, Kr, Xe, Rn) Don’t combine with any other elements

28
Q

Examples of Metals

A

Any Alkali metal, Alkaline Earth metal, or Transition metal

29
Q

Properties of Metals

A
  • High Electrical Conductivity
  • Shiny
  • Ductile
  • Malleable
30
Q

Metalloids

A

Are on the stair line

B, Si, Ge, As, Sb, Te, Po

31
Q

Properties of Metalloids

A

Properties of Metals and Non-Metals

  • shiny or no
  • ductile
  • can or cannot conduct electricity
32
Q

Properties of Non-Metals

A
  • Not Shiny
  • Don’t conduct electricity
  • Many are in GAS form
33
Q

Compare and Contrast Group A and Group B

A

Group A- Alkali Metals, Alkaline Earth Metals, Halogens, and Noble Gases
Group B- Transition Metals and Inner Transition Metals

34
Q

Examples of Alloy

A

any metal

35
Q

Compare and Contrast between Metallic, Covalent, and Ionic Bonds

A

Metallic bond hold METALS
Covalent bonds hold TWO NON-METALS
Ionic bonds held by negative or positive atoms or groups

36
Q

Molecule v Formula Unit

A

Molecule: Non-Metals CO2 NEED PREFIXES Carbon Dioxide

Formula Unit- A metal and Non-Metal NO Prefixes

37
Q

Formulas for the seven Diatomic Elements

A 
Hydrogen- H2
Oxygen- O2
Nitrogen- N2
Chloride- Cl2
Bromine- Br2
Iodine- I2
Fluoride- F2
38
Q

Formulas for Acids

A

ALWAYS H+
State- Aqueous (aq)
An Anion

39
Q

An Alloy

A

Two metals

40
Q

Charges on Alkali Metals, Alkaline Earth Metals, and Halogens

A

Alkali- +1
Alkaline- +2
Halogens- 3-

Chemistry ICA (4 decks)

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