Chem Ch 5 Test Flashcards

1
Q

What is the difference between periods and groups/families on the periodic table?

A

Period- left to right. Same number of electron orbitals
Groups- Up down. Same number of valence electrons

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2
Q

Who organized elements in groups of threes and fours based on similar properties?

A

Dobreiner

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3
Q

Newlands used what to organize the elements? Were his ideas accepted?

A

Atomic mass. No

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4
Q

What form of energy did Henry Moseley use to determine the atomic numbers of elements?

A

Frequency of x-ray

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5
Q

Which one of these is not an element symbol? O H HN Cu

A

HN

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6
Q

Transition metals occupy which numbered groups on the periodic chart?

A

Groups 3-12

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7
Q

Alkali metals occupy which numbered group on the periodic chart?

A

Group 1

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8
Q

Alkaline earth metals occupy which numbered group on the periodic chart?

A

Group 2

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9
Q

Noble gases occupy which numbered group on the periodic chart?

A

Group 18

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10
Q

Halogens occupy which numbered group on the periodic chart?

A

Group 17

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11
Q

Which side of the table do you find metals on left, right center or bottom?

A

Left and middle

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12
Q

Which side of the table do you find nonmetals on left, right center or bottom?

A

Right

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13
Q

Francium is in the lower left section of the periodic table, and Fluorine is in the upper right. Which has the larger atomic radius?

A

Francium

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14
Q

How does the size of a metal atom compare to its positive ion? Its negative ion?*

A

Positive (Cation)- Bigger
Negative (Anion)- Smaller

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15
Q

Ionization energy

A

Measures the energy required to remove an outermost electron

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16
Q

Magnesium is in Group 2 (2A) and Period 3 of the periodic table, and radium is in Group 2 (2A) and Period 7. Which has the smaller ionization energy?

17
Q

Which property measures the energy released when an electron joins an atom?
a. atomic size
b. ionic size
c. ionization energy
d. electron affinity
e. electronegativity

A

Electron affinity

18
Q

Property that measures the attraction of bonded atoms to electrons

A

Electronegativity

19
Q

A sample of an unidentified element has a bright luster, conducts electricity well, and is highly reactive. It is most likely what

A

Alkali metals

20
Q

Semiconductors can also be called __________. What do they do?

A

Metalloids. Conduct electricity but only under certain conditions

21
Q

The halogens form __________ when they combine with metals and __________ when they combine with hydrogen

A

Salts/acids

22
Q

What are examples of Halogens?.

A

Fluorine, Chlorine, Bromine, Iodine, Astatine,

23
Q

Who left blanks on his periodic table?

24
Q

Atomic radii does it increase or decrease as you go from left to right on the periodic table?
Why?

A

Decreases because more protons means more attraction for electrons. Results in shrinking of atomic radius

25
Atomic radii does it increase or decrease as you go from top to bottom on the periodic table? Why?
Increases because going down a group or family add extra layer of electrons for each level
26
Explain what is the trend in ionization energy going down a group and across a period. Also, explain why these trends are there.
Down decrease, further from nucleus easier to remove Right increase, closer to nucleus, more protons = more attraction, harder to remove
27
Electron affinity
Amnt of energy required to add electron to neutral atom to form negative ion Opposite of ionization energy
28
Electronegativity
Measure of attraction btwn nucleus and valence electrons Determined for atoms bonded in molecules
29
Alkaline Earth metals
Group 2 Denser, harder, higher melting points than alkali metals Typically donate 2 electrons Ex: Military flares, x-rays, bones
30
Transition metals
Shinier, harder, denser than groups 1&2 Some react easily some don’t Ex: coin, jewelry, wire
31
Inner transition metals
Paramagnetism- weak attraction to magnetic field Actinide series- highly radioactive Used in glass and atomic bombs
32
Post transition metals
Groups 13-16 Metalloids- characteristics lying between those of metals and nonmetals Semiconductors- conduct electricity under certain conditions
33
Boron family
Group 13 Boron- conducts electricity at high temps Aluminium- shiny, low density
34
Carbon family
Group 14 Nonmetal; no reactive at room temp Bond with anything 4 valence electrons
35
Oxygen family
Group 16 Exists as O2 and O3 Nonmetal- fairly nonreactive at room temp Colorless, odorless, tasteless Oxides and sulfites Sulfur- reactive at room temp
36
Halogen family
Group 17 More color, higher melting point, density Most reactive out of all nonmetals Used for halogen lights, bleach and medical uses
37
Noble gas family
Group 18 Colorless, odorless, tasteless Rarely react Used for balloons, diving, neon light
38
Nitrogen family
Normally diatomic gas Colorless, odorless, tasteless Phosphorus rarely found itself in nature Inert (doesn’t react)