Periodic table Flashcards

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1
Q

Periodic table

A

Elements in a table with order of increasing atomic number

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2
Q

Top of the f block (below transition metals)

A

Lanthanides

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3
Q

Bottom of f block(below transition metals)

A

Actinides

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4
Q

Properties of metals

A

Shiny solids, good conductors(heat+elec) malleable+ductile, generally high melting and boiling points, react with acid to give off hydrogen gas

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5
Q

Metalloids

A

zigzag down from B including Ge and Sb. Solid at room temp, not malleable or ductile, resist flow of electricity. When in chem reac with metals, they behave like nmetals. When in chem reac with nmetals they behave like metals.

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6
Q

Non metals

A

Dull, brittle, Insulators(Graphite is only exception - it is a conductor). Gaseous nmetals low melting + boiling points. Do not react with acids

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7
Q

Metallic nature decreases…

A

Across the period and increases down a group

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8
Q

Metal reactivity increases…

A

Down a group

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9
Q

Non metal reactivity increases…

A

Up a group

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10
Q

Density and melting points increase…

A

Down a group

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11
Q

Non metals become more metallic as…

A

Down a group

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12
Q

Ionization energy

A

Energy needed per mole to remove e- from an atom in gaseous phase

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13
Q

First Ionization energy

A

energy needed per mole to remove 1st e- from atom in gaseous phase.

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14
Q

Successive Ionization energy…

A

Requires increasing amount of energy to remove successive e- as a result of atom becoming progressively more positively charged from e removed.

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15
Q

Noble gases

A

High ionization energies due to full outer shell which explain why they dont react under normal circumstances

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16
Q

Causes of trends in io energy(not first io energy)

A

Valence electrons get further from nucleus resulting in weaker force of attraction require less energy to remove valence electron from atom and increased shielding effect - core electrons repel valence electrons. More core electrons down a group, shielding effect increases.

17
Q

Electron Affinity

A

Amount of energy released per mole when an atom or molecule gains an electron to form a negative ion. Halogens most likely to form negative ions. F has highest e affinitiy.

18
Q

Electronegativity

A

Tendency of atom to attract shared pair of e- to itself. More protons - stronger attraction on a bonding pair of electrons.

19
Q

Ion

A

Charged particle

20
Q

Cation

A

Positive ion - lost e-

21
Q

Anion

A

Negative ion - gained e-

22
Q

Atomic radius

A

Measure of size of atom

23
Q

Ionic radius

A

measure of size of cation or anion

24
Q

These increase from left to right across period and decrease as u go down group

A

Electronegativity, e- affinity and io energy

25
Q

Atomic and ionic radius trends

A

Bigger as u move down group and smaller across period