Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

10th grade > Chem Ch 5 Test > Flashcards

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

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

A

Dobreiner

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

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

A

Atomic mass. No

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

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

A

Frequency of x-ray

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

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

A

HN

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Transition metals occupy which numbered groups on the periodic chart?

A

Groups 3-12

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Alkali metals occupy which numbered group on the periodic chart?

A

Group 1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

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

A

Group 2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Noble gases occupy which numbered group on the periodic chart?

A

Group 18

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Halogens occupy which numbered group on the periodic chart?

A

Group 17

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

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

A

Left and middle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

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

A

Right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Ionization energy

A

Measures the energy required to remove an outermost electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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?

A

Radium

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?

A

Mendeleev

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
Q

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

A

Increases because going down a group or family add extra layer of electrons for each level

26
Q

Explain what is the trend in ionization energy going down a group and across a period. Also, explain why these trends are there.

A

Down decrease, further from nucleus easier to remove
Right increase, closer to nucleus, more protons = more attraction, harder to remove

27
Q

Electron affinity

A

Amnt of energy required to add electron to neutral atom to form negative ion
Opposite of ionization energy

28
Q

Electronegativity

A

Measure of attraction btwn nucleus and valence electrons
Determined for atoms bonded in molecules

29
Q

Alkaline Earth metals

A

Group 2
Denser, harder, higher melting points than alkali metals
Typically donate 2 electrons
Ex: Military flares, x-rays, bones

30
Q

Transition metals

A

Shinier, harder, denser than groups 1&2
Some react easily some don’t
Ex: coin, jewelry, wire

31
Q

Inner transition metals

A

Paramagnetism- weak attraction to magnetic field
Actinide series- highly radioactive
Used in glass and atomic bombs

32
Q

Post transition metals

A

Groups 13-16
Metalloids- characteristics lying between those of metals and nonmetals
Semiconductors- conduct electricity under certain conditions

33
Q

Boron family

A

Group 13
Boron- conducts electricity at high temps
Aluminium- shiny, low density

34
Q

Carbon family

A

Group 14
Nonmetal; no reactive at room temp
Bond with anything
4 valence electrons

35
Q

Oxygen family

A

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
Q

Halogen family

A

Group 17
More color, higher melting point, density
Most reactive out of all nonmetals
Used for halogen lights, bleach and medical uses

37
Q

Noble gas family

A

Group 18
Colorless, odorless, tasteless
Rarely react
Used for balloons, diving, neon light

38
Q

Nitrogen family

A

Normally diatomic gas
Colorless, odorless, tasteless
Phosphorus rarely found itself in nature
Inert (doesn’t react)

10th grade (71 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions