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Lydia's Brainscape Decks > Chemistry Unit 6 > Flashcards

Chemistry Unit 6 Flashcards

1
Q

Coulomb’s Law

A

When attraction goes up, then magnitude goes up and distance^2 goes down.

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2
Q

What is atomic radii?

A

Distance from the center of the nucleus to the boundary of the e- cloud.

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3
Q

Atomic radii group trend?

A

Larger, new energy levels of electrons. d^2 goes up, so attraction goes down. More e- shielding effect also weakening attraction of p+/ve- and increasing distance.

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4
Q

Atomic radii period trend?

A

Smaller, stronger positive to negative attraction from an increase in p+/ve-. Magnitude goes up, so attraction goes up (d^2 goes down).

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5
Q

Shielding Effect

A

The inner (core) electrons cause an interference and block the nucleus (p+) from the outer ve-. The more e-=more shielding effect.

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6
Q

What is first ionization energy?

A

The energy required to remove the most loosely held electron.

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7
Q

Ionization energy group trend?

A

Decreases, added energy level weakens attraction between p=/ve-. More Shielding effect. Easier to remove ve-. Coulombs: d^2 goes up, so attraction goes down.

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8
Q

Ionization energy period trend?

A

Increases, attraction between p+/ve- is greater, more protons(nuclear charge). Harder to remove e-. Coulombs: mag goes up, attraction goes up

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9
Q

Electronegativity

A

Attraction an atom has for a bonding pair of electrons (attract e- towards itself).

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10
Q

Electronegativity group trend?

A

Decreases, less attraction due to e- being further from nucleus. More shielding effect (bigger size). Coulombs: d^2 goes up, so attract goes down

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11
Q

Electronegativity period trend?

A

Increases, added p+/e- so greater attraction for e- (smaller size). Coulombs: magnitude goes up, attraction goes up.

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12
Q

What is reactivity?

A

How completely and easily an atom bonds to another (lose/gain/share).

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13
Q

Reactivity METALS group trend?

A

Increases, larger it is easier to lose e- due to distance and shielding effect.

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14
Q

Reactivity METALS period trend?

A

Decreases, smaller so hold on to e- is stronger due to more p+ and ve-.
Coulombs: magnitude goes up, attraction goes up.

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15
Q

Reactivity NONMETALS group trend?

A

Decreases, larger so less attraction to (others) ve-. Coulombs: magnitude goes up, attraction goes up.

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16
Q

Reactivity NONMETALS period trend?

A

Increases, smaller so more attraction to ve- and others. Coulombs: magnitude goes up, attract goes up.

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17
Q

Ionic size as compared to atom; which ANIONS and what is their trend?

A

(-), gained e- (not p+). NONMETALS larger because gained e-, e- repel other e- and expand. More (-) = larger anion. Cl is smaller and Cl^- is larger.

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18
Q

Ionic size as compared to atom; which CATIONS and what is their trend?

A

(+), lost e- (not p+), METALS smaller because lost electrons. Nucleus can pull e- in closer. more (+) = smaller cation. Fe is larger than Fe^+3.

19
Q

If we make all the atoms ions:

A

Same trend as atomic radii but it starts over at the staircase.

20
Q

are you ready for the test??

A

Keep studying!

21
Q

What ions do METALS form?

A

Cations (+)

22
Q

What ions do NONMETALS form?

A

Anions (-)

23
Q

What is the periodic law?

A

When arranged by increasing atomic number, there are chemical and physical properties that repeat periodically.

24
Q

What is a period?

A

Horizontal

25
Q

What is a group?

A

Vertical

26
Q

What are representative elements?

A

Elements in groups 1A-8A

27
Q

What did Dobereiner contribute?

A

“triad”- three elements with similar properties. Ex: Li, Na, K

28
Q

What did Newlands contribute?

A

Law of Octaves- Every 8th element, properties repeat. NOT octect rule: atoms gain or lose electrons to obtain 8 valence electrons.

29
Q

What did Meyer contribute?

A

Arrangement by atomic mass. Chemical properties repeat every so many elements.

30
Q

What did Mendeleev contribute?

A

Arrangement by INCREASING atomic mass. Predicted unknown elements by leaving spaces in the table. Germanium, Gallium, Scandium

31
Q

What did Moseley contribute?

A

Arrangement by increasing atomic number.

32
Q

Properties of METALS

A

small number of ve-, easily lose ve-, cations, good electrical and heat conductors, ductile, malleable, lustrous, solid at room temp

33
Q

Properties of NONMETALS

A

several ve-, anions, poor conductors of heat and electricity, non-ductile, brittle, not luster, s-l-g at room temp

34
Q

Properties of METALLOIDS

A

Both metal and nonmetal properties

35
Q

Properties of Alkali metals

A

soft, very reactive, stored under oil so they don’t react

36
Q

Properties of Alkaline earth metals

A

a little less soft, more mildly reactive, only react at temps when water is steam

37
Q

Properties of Halogens

A

Very smelly (ew!), burn flesh, does not dissolve well in water, reacts with most metals and many nonmetals

38
Q

Properties of noble gases

A

Not very reactive, do not like forming compounds with other elements, very stable

39
Q

Lanthanides

A

rare earth metals, similar across period, all solid

40
Q

Actinides

A

radioactive, similar across period, all solid

41
Q

Transition metals

A

contains everyday metals

42
Q

Malleable

A

bent or shaped easily

43
Q

Ductile

A

can be stretched into wire

44
Q

Atomic radius

A

Distance from the middle of the nucleus to the boundary of the electron cloud.

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