Chapter 2: Atoms and Elements Flashcards

1
Q

atomos

A

indivisible

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

atomic theory

A

all matter is composed of atoms

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

law of conservation of mass

A

in a chemical reaction, matter is neither created nor destroyed
- consistent with the idea that matter is composed of small, indestructible particles
when a chemical reaction occurs, the total mass of the substances involved in the reaction does not change

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

law of definite proportions (law of constant composition)

A

all samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements

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

law of multiple proportions

A

when two elements (call them A and B) form two different compounds, the masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers
- an atom of A combines with either one, two, three, or more atoms of B
- the ratio of these two masses is itself a small whole number

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

Dalton’s atomic theory

A
  • each element is composed of tiny, indestructible particles called atoms
  • all atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements
  • atoms combine in simple, whole-number ratios to form compounds
  • atoms of one element cannot change into atoms of another element. in a chemical reaction, atoms only change the way they they are bound together with other atoms
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

J.J. Thomson

A

proposed that the negatively charged electrons were small particles held within a positively charged sphere
- incorrect plum-pudding model

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

nuclear theory

A
  • most of the atom’s mass and all of its positive charge are contained in a small core called a nucleus
  • most of the volume of the atom is empty space, throughout which tiny, negatively charge electrons are dispersed
  • there are as many negatively charged electrons outside the nucleus as there are positively charged particles (named protons) within the nucleus, so that the atom is electrically neutral
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

neutrons

A

neutral particles within the nucleus

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

subatomic particles

A

protons, neutrons, electrons

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

proton

A

charge = +1

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

neutron

A

charge = 0

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

electron

A

charge = -1

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

atomic number

A

the number of protons in an atom’s nucleus

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

chemical symbol

A

either a one- or two-letter abbreviation listed directly below its atomic number on the periodic table

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

isotopes

A

atoms with the same number of protons but a different number of neutrons

17
Q

natural abundance

A

the percentages representing the relative amount of each different isotope in a naturally occurring sample of a given element is roughly constant

18
Q

mass number

A

the sum of the number of neutrons and protons in an atom

19
Q

ions

A

in chemical changes, atoms can lose or gain electrons and become charged particles called ____

20
Q

cations

A

positively charged ions, such as Na+

21
Q

anions

A

negatively charged ions, such as F-

22
Q

periodic law

A

when the elements are arranged in order of increasing mass, certain sets of properties recur periodically

23
Q

metals

A

lie on the lower left side and middle of the periodic table and share some common properties:
- good conductors of heat and electricity
- can be pounded into flat sheets (malleability)
- can be drawn into wires (ductility)
- often shiny
- tend to lose electrons when they undergo chemical changes

Chromium, copper, strontium, lead, etc.

24
Q

nonmetals

A

lie on the upper right side of the periodic table
- total of 17
properties:
- poor conductors of heat and electricity
- not ductile and not malleable
- gain electrons when they undergo chemical changes

Oxygen, carbon, sulfur, bromine, iodine, etc.

25
Q

metalloids/semimetals

A
  • elements that lie along the zigzag diagonal line that divides metals and nonmetals
  • exhibit mixed properties
  • several are also classified as semiconductors because of their intermediate (and highly temperature-dependent) electrical conductivity
26
Q

main-group elements

A

properties tend to be largely predictable based on their position in the periodic table

27
Q

transition elements (transition metals)

A

properties tend to be less predictable based simply on their position in the periodic table

28
Q

group/family

A

each vertical column of the periodic table

29
Q

period

A

each horizontal row of the periodic table

30
Q

noble gases

A

the group 8A elements that are mostly unreactive
- Helium is chemically stable - it does not combine with other elements to form compounds - and is therefore safe to put into balloons
- others include neon (often used in electronic signs), argon (a small component of our atmosphere), krypton, and xenon

31
Q

alkali metals

A

the group 1A elements that are all reactive metals
- sodium, lithium, potassium, and rubidium
– have a tendency to lose one electron and form 1+ ions

32
Q

alkaline earth metals

A

the group 2A elements that are fairly reactive, but not quite as reactive as the alkali metals
- calcium, magnesium, strontium, and barium
– tend to lose two electrons and form 2+ ions

33
Q

halogens

A

the group 7A elements that are very reactive nonmetals and always found in nature as a salt
- chlorine, bromine, iodine, and fluorine
– tend to gain one electron and form 1- ions

34
Q

oxygen family nonmetals

A

group 6A elements that tend to gain two electrons and form 2- ions

35
Q

mole (mol)

A

the measure of material containing 6.02214x10^23 particles:
- 1 mole = 6.02214 x 10^23 particles

36
Q

Avogadro’s number

A

6.02214x10^23 particles

37
Q

molar mass

A

the mass of 1 mol of atoms of an element