Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Chapter 6-Periodic Table > Flashcards

Chapter 6-Periodic Table Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Current periodic table is who’s model? What did he arrange the elements by?

A

Henry Moseley

atomic number

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

each box of the periodic table has…

A

element name
symbol
atomic number
atomic mass

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

period vs group

A

period: row
group: column

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

Representative elements

A

s and p blocks

possess wide range of chemical and physical traits

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

transition elements

A

d and f blocks

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

metals

A

usually solid at room temp

good heat and electricity conductors

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

Where are the metals located?

A

Left of staircase

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

Malleability

A

ability to be pounded thin

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

Ductility

A

ability to be drawn into wires

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

alkali metals

A

group 1 elements

very reactive
usually exist as compounds with other elements

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

alkaline earth metals

A

group 2 elements

very reactive

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

transition elements divided into ___ and ___

A

transition metals and inner transition metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

inner transition metals divided into ___ and ___, which are located in the ___ block

A

lanthanide series and actinide series

f block

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

nonmetals located…

A

right of staircase

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

nonmetals

A

usually gases or dull-looking solids

poor heat and electricity conductors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

which nonmetal is the only one that’s liquid at room temp?

A

bromine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

halogens

A

group 17

very reactive
often form compounds with other elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

noble gases

A

group 18

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

metalloids/semimetals

A

elements bordering staircase

physical and chemical traits of both metals and nonmetals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

only metal that is liquid at room temp?

A

Mercury

21
Q

counting valence e’s

A

look at s and p blocks (count in)

22
Q

noble gases have __ valence e’s each

A

8

23
Q

atomic radius

A

metals: 1/2 distance between a crystal’s adjacent nuclei
nonmetals: 1/2 distance between nuclei of identical atoms

24
Q

trend of atomic radii from left to right

A

decrease

# of protons increase from left to right
more protons have stronger pull on negative e's (increased positive charge on nucleus)
atoms become more constrained
25
Q

trend of atomic radii down a column

A

increase

more energy levels
although there are more e’s, they’re further away from the nucleus (less pull=less constraint)

26
Q

ion

A

formed when atom gains or loses e’s

27
Q

ionic radius: lose electrons

A

becomes smaller

e’s lost (possible empty orbital)
nucleus pulls remaining e’s closer

28
Q

ionic radii trend: period (left to right)

A

positive ions decrease from groups 1-13

neg ions decrease from groups 14-17

29
Q

ionic radii trend: groups

A

increases going down

30
Q

ionization energy

A

energy needed to remove valence e

31
Q

ionization energy trend in a period (left to right)

A

increases

elements on right want to gain e’s since they are closer to achieving the octet
stronger pull

32
Q

ionization energy trend down a group

A

decreases

atomic radius increases
less pull

33
Q

octet rule

A

atoms tend to gain, lose, or share e’s in order to get a full set of 8 valence e’s

34
Q

electronegativity

A

ability to attract e’s in a chemical bond

35
Q

types of ions

A

cation

anion

36
Q

cation

A

positive (lost e)
metals
smaller than original atom

37
Q

anion

A

negative, gain e
nonmetals
larger than original atom

38
Q

shielding

A

e’s between nucleus and valence shell shield pull on valence e’s

39
Q

ditomic elements

A

7, make a 7 in periodic table
always occur in pairs in nature (ex. N2, O2)

top of 7 starts at NOF

40
Q

periodic law

A

there’s a periodic repetition of chemical and physical properties of elements when arranged by increasing atomic #

41
Q

shielding effect trend: period

A

constant

42
Q

shielding effect trend: group

A

increases from top to bottom

more energy levels

43
Q

why are valence e’s not shielded from the increasing positive nuclear charge as atomic radius increases across a period?

A

no e’s (energy level n) come between the nucleus and valence e’s

44
Q

second ionization energy

A

removing the 2nd e

requires more energy

45
Q

why is the octet rule useful?

A

used for predicting what types of ions an element will form

46
Q

Which block is He a part of?

A

s

47
Q

Why do elements in the same group have similar chemical properties?

A

same # of valence e’s

48
Q

valence e configuration

A

last part of normal e configuration

shows the # of valence e’s

49
Q

determining # of valence e’s for representative elements

A

s and p block (count in)

Chemistry (5 decks)

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