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Honors Chemistry > Periodic Table and Trends > Flashcards

Periodic Table and Trends Flashcards

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1
Q

What are the columns of elements in the periodic table?

A

Groups

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2
Q

What are rows of elements in the periodic table?

A

Periods

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3
Q

A family of elements is the same as…

A

A group

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4
Q

A metal can be stretched into thin wire is…

A

Ductile

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5
Q

The ability to conduct electricity is a property of…

A

Metals

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6
Q

A metal that can be hammered into thin sheets because it is…

A

Malleable

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7
Q

A property of metals is ____ or shininess.

A

Luster

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8
Q

______ is the gradual wearing away of a metal due to a chemical reaction with water or elements in the atmosphere.

A

Corrosion

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9
Q

Elements that are ______ are located to the right of the zig-zag line in the periodic table.

A

Nonmetals

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10
Q

Elements that have the same properties as both, metals and nonmetals are…

A

Metalloids

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11
Q

______ are elements that tend to gain electrons in chemical reactions.

A

Nonmetals

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12
Q

Coulombic Attraction

A

The attraction between oppositely charged particles.

less distance, more attraction; more distance, less attraction

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13
Q

Number of protons + attractive force

A

Increased protons –> increased attractive force

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14
Q

Electrons are attracted to protons in a nucleus, but are repelled by electrons in the same atom.

A

Electron Repulsion

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15
Q

Ion

A

An atom that is negatively/positively charged, or neutral.

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16
Q

Valence electron

A

Electrons in the outermost shell of an atom.

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17
Q

How is an ion formed?

A

When an atom gains/loses an electron to reach stability

18
Q

Ionization energy

A

Energy required to remove an electron

19
Q

Ionic Radius

A

The size of an ion, when it gains/loses an electron.

20
Q

Cation

A

Positively charged ion - neutral ion is larger than (>) +ion
Na+
- less electrons -> less repulsion
- # of shells dec. -> stronger attraction towards valence electrons
- less shielding effect

21
Q

Anion

A

Negatively charged ion - neutral ion is smaller than ( more electron repulsion
- same shielding effect

22
Q

Shielding Effect

A

Describes the balance between the pull of the protons on valence electrons and the repulsion forces from inner electrons

23
Q

Atomic Radius

A

The size of an atom

  • The distance between the nucleus and valence electrons
  • 1/2 distance between the nuclei
24
Q

Atomic Radius - across a period

A

Atomic radius DECREASES

  • proton # increases, attraction increases
  • distance stays the same -> same period = same # of shells
  • shielding effect stays the same
  • electron repulsion increases, but not as effective
25
Q

Atomic Radius - down a group

A

Down a group, atomic radius increases

  • distance between valence electrons and nucleus increases -> # of shells increase
  • shielding effect increases, attraction decreases
  • electron repulsion increases (makes atom larger)
26
Q

Electronegativity

A

The tendency for an atom to attract shared electrons when forming a chemical bond.

  • element with the highest electronegativity: F (Fluorine) (approx 3.98 or 4.0)
  • G18 ARE NONMETALS - DO NOT ATTRACT
27
Q

Electronegativity - across a period

A
  • Across a period, increases
  • Atoms get smaller
  • Proton # increases, distance stays the same
  • Attraction towards electrons increase
  • Electronegativity increases
28
Q

Electronegativity - down a group

A
  • Down a group, electronegativity decreases
  • Atoms are getting larger
  • Attraction gets weaker
  • Less attraction, towards electrons
  • Electronegativity decreases
29
Q

Reactivity

A

A measure of how readily a substance undergoes a chemical reaction

30
Q

Reactivity: Metals - down a group

A
  • Down a groups, reactivity increases for metals.
  • Starts to form positive ions
  • Wants to lose electrons
  • Less force of attraction - valence electrons
  • Less ionization energy -> easier to remove an electron
  • Easier to react to other elements
31
Q

Reactivity: Metals - across a period

A
  • Across a period, reactivity decreases for metals.
  • More attraction for valence electron
  • More ionization energy -> harder to remove an electron
  • Harder to react with other elements
  • Most reactive metal: Francium
32
Q

Reactivity: Nonmetals - down a group

A
  • Down a group, reactivity decreases for nonmetals.
  • Forms negative ions
  • Wants to gain electrons
  • Less attractions - valence electrons
  • Less electronegativity
  • Lower reactivity
33
Q

Reactivity: Nonmetals - across a period

A
  • Across a period, reactivity increases in nonmetals.
  • More attraction for valence electrons
  • More electronegativity
  • Higher reactivity
  • Most reactive NM: Chlorine
34
Q

Alkali Metals

A
  • GROUP 1, does not include hydrogen
  • Shiny, soft, highly reactive metals
  • DO NOT OCCUR NATURALLY
  • Only have 1 valence electron
  • Reactivity increases down the group
35
Q

Alkaline Earth Metals

A
  • GROUP 2
  • Has 2 valence electrons
  • Somewhat reactive metals, some of which occur naturally as free elements
  • Reactivity increases down the group
36
Q

Icosagens

A
  • GROUP 3
  • All have 3 valence electrons
  • Called “poor metals” due to their low melting points + hardness
  • Liquid at a larger range of temperature than any other element
37
Q

Crystallogens

A
  • GROUP 4
  • A mix of metals, nometals, and metalloids
  • All have 4 valence electrons
38
Q

Pnictogens

A
  • GROUP 5
  • All have 5 valence electrons
  • All solids, apart from nitrogen, are a mix of nonmetals, metalloids and metals
39
Q

Chalcogens

A
  • GROUP 6
  • All have 6 valence electrons
  • Form -2 ions when reacting w/ electropositive metals
40
Q

Halogens

A
  • GROUP 7
  • Contains elements in all 3 states of matter
  • All reactive nonmetals
  • All form diatomic molecules
  • Reactivity decreases down the group
41
Q

Noble Gases

A
  • All monoatomic, rarely form compounds

- Not very reactive -> already have a full valence electron shell

Honors Chemistry (4 decks)

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