chap 6 Flashcards

1
Q

going down a group of the periodic table what patterns would you notice?

A
  • atomic size increases
  • ionic size increases
  • ionization enegry decreases
  • electronegativity decreases
  • nuclear charge increases
  • shielding increases
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Going across a period what patterns would you notice?

A
  • Atomic size decreases
  • ionization energy increases
  • electronegativity increases
  • nuclear charge increases
  • shielding is constant
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

elements were first classified according to what

A

their properties

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

who created the periodic table

A

Mendeleev

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

on mendeleevs periodic table how were elements placed

A

in increasing atomic mass

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

what did Mendeleev discover thru his table

A

the properties of unknown elenments

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

what is the modern day table organized by

A

atomic number

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

metals are…

A

good conductors and many are ductile and malleable

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

nonmetals are…

A

mostly gase whose properties are opposite to those of metals

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

metaloids can…

A

behave like metals or nonmetals depending on condition

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

How many elements had been identified by the year 1700?

A

13

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

What caused the rate of discovery to increase after 1700?

A

Chemists began to use scientific methods to search for elements

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

What did chemists use to sort elements into groups?

A

Chemists used the properties of elements.

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

Who was Dmitri Mendeleev?

A

he created a periodic table

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

What property did Mendeleev use to organize the elements into a periodic table?

A

arranged the elements in order of increasing atomic mas

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

what are 3 things u can name by looking at an element on the periodic table

A
  • atomic number
  • atomic mass
  • what type of element it is
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what is a valence electron

A

outer edge

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

Why are Group A elements called representative elements?

A

They exhibit a wide range of physical and chemical properties

19
Q

Description of Electron Configuration for noble gases

A

s or p sublevels are filled

20
Q

Description of Electron Configuration for Representative elements

A

s or p sublevels are only partially filled

21
Q

Description of Electron Configuration for transition metals

A

s sublevel and nearby d sublevel contain electrons

22
Q

Description of Electron Configuration for inner transition metals

A

s sublevel and nearby f sublevel contain electrons

23
Q

letter of the elements found in the p block

A

Groups 3A, 4A, 5A, 6A, 7A, and 8A except helium

24
Q

Ions form when…

A

atoms gain or lose electrons.

25
A positively charged cation forms
when an atom loses one or more electrons.
26
negatively charged anion forms
s when an atom gains one or more electrons.
27
First ionization energy
is the amount of energy required to remove one electron from a neutral atom
28
Ionization energy tends to decrease from
top to bottom within a group an increase from left to right across a period.
29
A cation is
smaller than the atom that formed it
30
an anion
is larger than the atom that formed it.
31
Ionic size generally increases
from top to bottom within a group
32
Ionic size generally decreases
from left to right across a period.
33
Electronegativity tends to decrease from
top to bottom
34
Electronegativity tends to increase from
from left to right across a period.
35
What is the general trend in atomic size within a group?
The atomic size increases within a group as atomic number increases. The atomic size decreases from left to right across a period
36
What are the two variables that affect atomic size within a group?
- the charge on the nucleus - the number of occupied energy levels
37
What is an ion?
an atom or group of atoms that has a positive or negative charge
38
How are ions formed
An ion is formed when electrons are transferred between atoms.
39
An ion with a positive charge is called a(n)
cation
40
an ion with a negative charge is called a(n)
anion
41
anions
- neg - nonmetal - minus sign
42
cations
- pos - metal - plus sign
43
Why does ionization energy tend to decrease from top to bottom within a group?
Atomic size increases from top to bottom within a group. The nuclear charge has a smaller effect on the electrons in the highest occupied energy level, so less energy is required to remove an electron.