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CHEM 1210 > Chapter 7: Periodic Properties of the Elements > Flashcards

Chapter 7: Periodic Properties of the Elements Flashcards

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1
Q

Are (aq) metal oxides usually acidic or basic?

A

basic

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2
Q

What phase are MOLECULAR compounds usually found in at room temp?

A

gas…or sometimes, liquids

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3
Q

How/why are (aq) metal oxides basic?

A

The O2- reacts with H2O to form OH- (which is attached to the metal)

CaO + H2O = Ca(OH)2

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4
Q

Which group 1 (alkali) metal is the only one that does NOT make hydrogen peroxide with oxygen?

A

Li

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5
Q

Which way does atomic radius trend across the periodic table?

A

Gets bigger as you go down and to the LEFT

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6
Q

Which energy level (high, med, low, etc) do metals loose electrons from FIRST when they ionize/become cations?

A

The highest energy level

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7
Q

Under what circumstances does loosing an electron cause an element to ABSORP energy?

A

when losing the electron INCREASES the number of unpaired electrons in a given subshell OR when losing an electron results in adding electrons to a previously empty subshell with higher energy

this is energetically UNfavorable

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8
Q

What does it mean for an element to have a positive electron affinity value?

A

it means that gaining an electron is energetically UNfavorable

energy is required in order to gain this electron

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9
Q

Which 3 noble gases have been shown to make compounds?

A

Xe, Kr, and Ar

Ar you Kr(ay) Xe?!

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10
Q

What 3 compound can Xe make with F?

A

XeF2, XeF4, and XeF6

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11
Q

What does sulfur usually form (with other elements)?

A

sulfides

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12
Q

Why does ionization energy go DOWN as elements get bigger?

A

when valence electrons are farther away from the nucleus (as in an element with a large atomic radius), they are easier to remove

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13
Q

What’s the best/easiest way to determine if a material has metallic quality?

A

By the material’s first ionization energy/If the material easily becomes a cation/gives up electron(s)

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14
Q

Do atoms get bigger or smaller when they become anions?

A

bigger

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15
Q

Does ionization energy apply to solids, liquids, or gasses?

A

gasses

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16
Q

Is ionization energy always endothermic or always exothermic

A

exothermic

some amount of energy is always required to remove en electron from an element/compound endothermic

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17
Q

Which two group 17 halogens are allotropic elements?

A

oxygen and sulfur

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18
Q

Can an insoluble metal oxide still participate in a neutralization reaction?

A

Yes. If acid is present, the metal oxide can still act like a base and participate in neutralization

This is true even though the insoluble metal oxide won’t dissociate in pure water.

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19
Q

How does the energy level (n value) of a given electron impact it’s first ionization energy?

A

Electrons in higher energy levels (with higher n values) are easier to remove that electrons in lower energy levels (because the high level electrons are further away/better shielded from the attractive force of the nucleus)

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20
Q

What do group 7 ions usually make with metals?

A

ionic metal halides

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21
Q

What is the equation for nuclear effective charge (Zeff)?

A

Zeff = number of protons (Z) - number of core electrons (S)

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22
Q

Which is more important for the trend in ATOMIC RADIUS: up & down or left to right?

A

up and down

23
Q

Are NON metals usually acidic or basic?

A

Acidic

24
Q

What compound can Ar make with H and F?

A

HArF

25
Q

What do group 1 (alkali) metals make with non-metals?

A

ionic compounds (like metal hydride or metal sulfide)

26
Q

Why does ionization energy go up as radius goes down/gets smaller?

A

As the elements get smaller, their valence electrons are closer to the nucleus/more attracted to the nucleus/feel more Zeff. This makes them harder to remove

27
Q

What kind of ‘oxides’ do group 1 (alkali) metals usually make with oxygen?

A

metal PERoxides (most of the time; like with Sodium),

metal oxides (sometimes; like with Lithium),

super peroxides (rarely, like with potassium)

28
Q

Isoelectric Series

A

a series of ions that has the same number of electrons

Sizes of these atoms decreases with increasing nuclear charge (bc the electrons are more attracted to the nucleus)

29
Q

Which way do ionization energy and electron affinity trend across the periodic table?

A

Get bigger as you go up and to the right

30
Q

Under what circumstances does loosing an electron cause an element to release energy?

A

when losing the electron reduces the number of unpaired electrons in a given subshell OR when losing an electron results in the emptying of a higher subshell when losing an electron brings the atom to having a half-full shell

this is energetically favorable

31
Q

Which is more important for the trend in Zeff: up & down or left to right?

A

left to right (bc left to right, you are adding protons but not adding additional core electrons to shield the valence electrons from the additional protons)

32
Q

What does it mean for an element to be allotropic?

A

that the element can exist in different forms, in the same state (like 02 and O3 ozone)

33
Q

How/why are (aq) NONmetal oxides acidic?

A

they combine with water to make acids

CO2 + H2O = H2CO3

34
Q

what do metal OXIDES form with acids?

A

salt and water

35
Q

What do you call the ion that elemental oxygen becomes (for bonding)?

A

peroxide ion

36
Q

Why is the trend in Zeff more pronounced left to right rather than up to down?

A

because from left to right, more protons are being added, but no new core electrons are being added to shield the valence electrons from the nucleus.

This causes the Zeff to increase

37
Q

When do you need to worry about calculating/estimating Zeff with the Zeff equation?

A

When you’re comparing the Zeff of multiple elements or compounds and you have to consider their charges AND their sizes.

38
Q

Do group 17 non-metals (halogens) tend to be alone or in compounds?

A

They tend to be in compounds and will bind with most metals

39
Q

What phase are ionic compounds usually found in at room temp?

A

solid

40
Q

What does it mean for an element to have a NEGATIVE electron affinity value?

A

it means that gaining the electron is energetically favorable; energy is released when the electron is gained

41
Q

Are (aq) NONmetal oxides usually acidic or basic?

A

acid

42
Q

Metallic Character

A

Tendency of an element to exhibit the properties of metals

43
Q

What does oxygen usually form (with other elements)?

A

oxides

44
Q

What do NONmetal oxides form with water?

A

acid (like a combination reaction)

45
Q

Do atoms get bigger or smaller when they become CATions?

A

smaller

46
Q

What do group 1 (alkali) metals make with water?

not the same thing as metal oxides

A

metal hydroxide (base) and H2 gas

47
Q

Which way does effective nuclear charge trend across the periodic table?

A

Gets bigger as you go down and to the right

48
Q

What do NONmetal oxides form with bases?

A

salt and water (like a neutralization)

NiO + 2 HNO2 = Ni(NO3)2 + H2O

49
Q

What does hydrogen ion form with non-metals?

A

molecules/molecular compounds

50
Q

What compound can Kr make with F?

A

KrF2

51
Q

Does low first ionization energy make an atom more reactive, or less reactive?

A

more reactive

52
Q

True or false: alkali metals only exist in nature as part of compounds

A

true; this is why they will always try to combine with other things…(generally, non metals, so they can form ionic compounds)

53
Q

what is the symbol/charge for peroxide ion?

A

O2 ^2-

CHEM 1210 (18 decks)

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