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Chemistry 112 > Chem 112 (Review) - Chp 6 > Flashcards

Chem 112 (Review) - Chp 6 Flashcards

1
Q

What is another name for the representative elements?

A

Group A/main group elements

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2
Q

What is another name for the transition metals?

A

D Block Elements

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3
Q

Which elements are in the same period as phosphorus?

A

Na, Mg, Al, Si, P, S, Cl, and Ar

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4
Q

The modern period table is arranged in order of atomic “ “

A

Number

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5
Q

Who arranged the elements according to atomic mass and use the arrangement to predict the properties of missing elements?

A

Dmitri Mendeleev

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6
Q

Which general category of elements includes the majority of elements?

A

Metals

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7
Q

Of the elements Pt, V, Li, and Kr which are a nonmetal?

A

Kr is a nonmetal element.

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8
Q

To what category of elements does an element belong if it is poor conductor of electricity?

A

Nonmetals

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9
Q

In which of the following sets is the symbol of the elements, the number of protons, and the number of electrons given correctly?

A

(a) In - 49 protons and 49 electrons
(b) Zn - 30 protons and 60 electrons
(c) Cs - 55 protons and 132.9 electrons
(d) F - 19 protons and 19 electrons

                  *ANSWER: A*
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10
Q

The atomic number of an element is the total number of which particle in the nucleus?

A

Protons

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11
Q

What element has the electron configuration of 1s2, 2s2, 2p6, 3s2, 3p2?

A

Silicon (Si)

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12
Q

What is true about electron configurations of all noble gases?

A

The highest occupied sublevels “s” and “p” are completely filled

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13
Q

Where can you find the representative elements on the periodic table?

A

1 & 2 and 13-18

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14
Q

How does atomic radius change from top to bottom in a group in the periodic table?

A

Going down, it will increase.

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15
Q

How does atomic radius change from left to right across a period in the periodic table?

A

Decreases from left to right.

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16
Q

What causes the shielding effect to remain constant across a period?

A

The number of energy levels are the same.

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17
Q

What element in the second period has the largest atomic radius?

A

Lithium (Li)

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18
Q

What is the charge of a cation?

A

A positive charge

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19
Q

How are cations formed?

A

When an atom/compound loses, one or more electrons.

20
Q

How are anions formed?

A

When an atom gains one or more electrons.

21
Q

What are the charges of ions formed from the following elements? Na, Mg, Al, N, O.

A

Na: 1
Mg: 2
Al: 13
N: 15
O: 16

22
Q

What is the element with the lowest electronegativity value?

A

Francium

23
Q

What is the element with the highest electronegativity value?

A

Fluorine

24
Q

What is the energy required to remove an electron from an atom in the gaseous state called?

A

Ionization energy

25
Q

Which of the following elements has the smallest first ionization energy?

A

(a) sodium
(b) calcium
(c) potassium
(d) magnesium

ANSWER: C

26
Q

Which of the following elements has the lowest electronegativity?

A

(a) lithium
(b) carbon
(c) bromine
(d) fluorine

ANSWER: A

27
Q

Which statement is true about electronegativity?

A

(a) electronegativity is ability of an anion to attract another anion.
(b) electronegativity generally increases as you move top to bottom with a group.
(c) electronegativity generally is higher for metals than for nonmetals.
(d) electronegativity generally increases from left to right across a period.

ANSWER: D

28
Q

Which of the following decreases with increasing atomic number and group 2A?

A

(a) shielding effect
(b) ionic size
(c) ionization energy
(d) number of electrons

29
Q

What happens to the relative size of an atom when it becomes a cation?

A

becomes SMALLER than the atom

30
Q

What happens to the relative size of an atom when it becomes a anion?

A

becomes a LARGER atom

31
Q

Which group of elements in the periodic table is known as the alkali metals?

A

Group 1A

32
Q

Which group in the periodic table is known as noble gases?

A

Group 18

33
Q

An element has atomic number of 80. How many protons and electrons are in an atom of the elements?

A

80 protons and 80 electrons (equal)

34
Q

What is the electron configuration of oxygen?

A

1s2 , 2s2 , 2p4 : Oxygen

35
Q

What is the electron configuration of sulfur?

A

[Ne] 3s2 and 3p4 : Sulfur

36
Q

The “S” and “P” sublevels of an atom of an element in period three are filled with electrons. Which orbitals are filled in this atom?

A

3s and 3p

37
Q

What orbital is filled with iodine gains an electron to become a negative ion?

A

5p orbital

38
Q

How many electrons are present in the D sub level of a neutral atom of nickel?

A

8 electrons in the “D” orbital

39
Q

How many electrons are in rubidium ion (Rb+)?

A

37 electrons

40
Q

What is the usual charge on an ion from group 7A?

A

Charges “-1”

41
Q

How many electrons does the ion Ca2+ contain?

A

18 electrons
(20-2=18)

42
Q

Explain how ions form. Provide examples.

A

When an atom gains/loses electrons in order to find a more stable configuration.

-> chlorine takes an electron from sodium, then sodium gives the electron chlorine that creates “NaCl”

43
Q

What is electronegativity? Describe the trends in electronegativity within groups and across periods in the periodic table. Provide examples.

A

The ability of an atom to attract electrons when the atom is in a compound.

-> INCREASES when moving left to right and DECREASES as you move down in a group.

44
Q

How do they measure atomic radius? Why does the atomic radius decrease as you move across the periodic table?

A

Atomic radius is measured in picometers (1x10^-12)

-> valence electrons are being added to the same energy level at the same time. The nucleus is INCREASING in protons.

45
Q

What does ionization energy mean? For the elements in group 2A, compare the relative values of their first, second and third ionization energy and explain why this is.

A

Energy that is required to remove an electron from an atom in its gaseous state.

-> first - low
-> second - high
-> third - highest

Chemistry 112 (7 decks)

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