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Chemistry > Chapter 4: Chemical Foundations: Elements, Atoms and Ions > Flashcards

Chapter 4: Chemical Foundations: Elements, Atoms and Ions Flashcards

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1
Q

Which element includes the first letter of its name as the first letter of the symbol for the element?

A.potassium
B. lead
C. copper
D.sodium

A

Copper

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2
Q

Which of the following postulates of Dalton’s atomic theory is no longer scientifically accepted?

A. All matter is made up of atoms.

B. All atoms of the same element are identical.

C. Compounds are combinations of different atoms.

D. Chemical reaction changes the way atoms are grouped.

A

B - All atoms of the same element are identical

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3
Q

Consider isotopes, ions, protons, and electrons. How many of these did Dalton not discuss in his atomic theory?

A.1
B. 2
C. 3
D.4

A

D - 4

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4
Q

Which of the following represents a pair of isotopes?

A

C

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5
Q

An ion is formed

A. Either by adding or by taking away protons from the atom.

B. either by adding or by taking away electrons from the atom.

C. either by adding or by taking away neutrons from the atom.

D. At least two of the above statements correctly explain how an ion is formed.

A

B - either by adding or by taking away electrons from the atom

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6
Q

How many protons and electrons does the most stable ion for oxygen have?

A.10 protons, 8 electrons

B. 8 protons, 8 electrons

C. 8 protons, 10 electrons

D.6 protons, 8 electrons

A

C. 8 protons, 10 electrons

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7
Q

A certain ion has a charge of 21 and 27 electrons. Which ion is it?

A

B

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8
Q

You are given a compound with the formula CaX2, in which X is a nonmetal. You are told that the nonmetal ion has 10 electrons. What is the symbol of the nonmetal?

A.F
B.Cl
C.O
D.Ne

A

A – F

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9
Q

______ Noble gases
______ Alkaline earth metals
______ Halogens
______ Alkali metals

A

d – noble gases
a – Alkaline earth metals
b – Halogens
c – Alkali metals

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10
Q

Briefly describe Ernest Rutherford’s gold foil experiment. Answer the following questions in your explanation.

A. What did Rutherford do?

B. What were the results?

C. What did Rutherford conclude from these results?

A

a - Rutherford “shot” alpha particles (helium nuclei) at thin gold foil.

b - Rutherford found that most of the alpha particles went through the gold foil but that some particles were deflected

c - Rutherford concluded that because the alpha particles are relatively heavy and positively charged and a small number were deflected, there must be a small, massive, positively charged part of an atom. He termed this the nucleus.

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11
Q

Review Isotopes Pogil!

A
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12
Q

Describe Dalton’s Atomic Theory, 3 key take aways…

A

1 – Elements consist of indivisible small particles (atoms).

2 – All atoms of the same element are identical; different elements have different types of atom.

3 – Atoms can neither be created nor destroyed.

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13
Q

What is the law of Constant Composition?

A

A given compound always has the same proportion by mass of the elements of which it is composed.

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14
Q

Regarding Dalton’s Atomic Theory

True or False:

Elements are made of tiny particles called atoms

A

True

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15
Q

Regarding Dalton’s Atomic Theory

True or False:

All atoms of a given element are identical

A

False

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16
Q

Regarding Dalton’s Atomic Theory

True or False:

A given compound always has the same relative numbers and types of atoms

A

True

17
Q

Regarding Dalton’s Atomic Theory

True or False:

Atoms are indestructible

A

False

18
Q

What are the 3 rules for writing formulas of compounds?

A
  1. Each atom present is represented by its element symbol.
  2. The number of each type of atom is indicated by a subscript written to the right of the element symbol.
  3. When only one atom of a given type is present, the subscript 1 is not written.
19
Q

What are Isotopes?

A

Isotopes are atoms with the same number of protons but different number of neutrons

20
Q

What the heck is this thing? Identify it’s bits:

What does the mass number represent?

What does the atomic number represent?

A

A. Mass Number = The sum of Protons and Neutrons

Z. Miss Atomic Bomb Number = Number of Protons

X. element symbol

21
Q

Describe some important features of subatomic particles.

A

Subatomic particles include electrons, the negatively charged, almost massless particles that nevertheless account for most of the size of the atom, and they include the heavier building blocks of the small but very dense nucleus of the atom, the positively charged protons and the electrically neutral neutrons.

22
Q

Describe the parts of an atom.

A

Atoms consist of three basic particles: protons, electrons, and neutrons.

The nucleus (center) of the atom contains the protons (positively charged) and the neutrons (no charge).

The outermost regions of the atom are called electron shells and contain the electrons (negatively charged).

23
Q

The Periodic Table shows all the known elements in order of _______________.

The Periodic Table is organized to group elements with similar properties in __________________.

A

Increasing Atomic Number.

Vertical Columns.

24
Q

The Periodic Table:

Most elements are __________ and occur on the _________ side.

Nonmetals appear on the ________ side.

Metalloids are elements that have some ___________ and some __________ properties.

A

Most elements are METALS and occur on the LEFT side.

Nonmetals appear on the RIGHT side.

Metalloids are elements that have some METALLIC and some NONMETALLIC properties.

25
Q

Name the 4 Physical Properties of Metals

A
  1. Efficient conduction of heat and electricity
  2. Malleablility
  3. Ductility
  4. A lustrous (shiny) appearance
26
Q

Name the 7 Diatomic Elements:

A

Hydrogen

Nitrogen

Oxygen

Fluorine

Chlorine

Bromine

Iodine

27
Q

Let’s talk Ions:

Atoms can form ions by ___________ or ____________ electrons.

Metals tend to lose one or more electrons to form ____________ ions called ___________.

Nonmetals tend to gain one or more electrons to form _________ ions called _________.

__________ are generally named by using the name of the ________ atom.

________ are named by using the root of an atom name followed by the suffix -_________.

Ionic Compounds are electronically ____________.

A

Atoms can form ions by GAINING or LOSING electrons.

Metals tend to lose one or more electrons to form POSITIVE ions called CATIONS.

Nonmetals tend to gain one or more electrons to form NEGATIVE ions called ANIONS.

CATIONS are generally named by using the name of the PARENT atom.

ANIONS are named by using the root of an atom name followed by the suffix -IDE.

Ionic Compounds are electronically NEUTRAL.

28
Q

The charges of the Anions and Cations in the compound must sum to __________.

A

Zero.

(they be neutral compounds)

29
Q

How can we use the periodic table to Predict which ion a given element forms?

A

Elements in Group 1A and Group 2A form 1+ and 2+ ions

Group 7A atoms form anions with 1 - charges

Group 6A atoms form anions with 2 - charges

Chemistry (6 decks)

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